Thermodynamics, Equilibrium and 2 other Topics - Maths - MCQ Test

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Thermodynamics, Equilibrium and 2 other Topics

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Jan 09, 8:00 AM

200 minutes

Jan 09, 11:20 AM

500.0 marks

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Thermodynamics, Equilibrium and 2 other Topics

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MCQ Test of 11, Maths & Biology & Chemistry & Physics & Hindi & English Thermodynamics, Equilibrium and 2 other Topics - Study Material

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Question 2 : Assertion: A buffer solution has a capacity to resist the change in pH value on an addition of a small amount of acid or base to it. Reason: An aqueous solution of ammonium acetate can act as buffer.

Question 3 : The $pH$ of the given solution of lactic acid and lactate is 4.30. Calculate the $pKa$ of lactic acid, when the concentration of lactic acid and lactate are 0.020M and 0.073M respectively.

Question 6 : Addition of water to this solution will not change $[H_3 O^+]$.

Question 8 : Match List-1 with List-2.<div> <table class="table table-bordered"><tbody><tr><td> List -1 </td><td> List-2</td></tr><tr><td> A) Aq. Solution of NaCl </td><td> 1)Acidic buffer</td></tr><tr><td> B) Aq. Solution of $CH_3COONa$ </td><td> 2)Acidic solution</td></tr><tr><td> C) Aq. Solution of $NH_{4}Cl$ </td><td> 3) Basic solution</td></tr><tr><td> D) Aq. Solution of $CH_{3}COOH$ along with $CH_{3}COONa$</td><td> 4)Neutral solution</td></tr></tbody></table> </div>

Question 10 : Which of the following will produce a buffer solution when mixed in equal volumes?

Question 11 : Calculate the PH of a buffer solution prepared by dissolving 30g of $Na2CO3$ in 500 ml of an aqueous solution containing 150 ml of 1m $HCL$. ka for $HCO^{-3}$ = 5.63 x 10-11

Question 12 : To prepare a buffer of pH 8.26 amount of $({ NH }_{ 4 }{ ) }_{ 2 }{ SO }_{ 4 }$ to be added to 500 mL of 0.01 M ${ NH }_{ 4 }OH$ solution is : $[pK_{ a }({ NH }_{ 4 }^{ + })\ =9.26]$

Question 13 : The $p{ K }_{ a }$ of acetylsalicyclic acid (asprin) is $3.5$. The pH of gastric juice in human stomach is about 2-3 and the pH in the small intestine is about $8$. Asprin will be:

Question 14 : Which of the following salt solution will act as a buffer?

Question 15 : Which of the following solution mixture will show resistance to the small addition of acids?

Question 16 : Which one of the following pairs of solution is not an acidic buffer?

Question 17 : $K_a (HCN)$ is $5\times { 10 }^{ -10 }$ at ${ 25 }^{ \circ }C$. For maintaining a constant pH of 9, the volume of 5M $KCN$ solution required to be added to 10mL of 2M $HCN$ solution is:

Question 18 : If $0.00050$ mol $NaH{CO}_{3}$ is added to $1$ litre of a buffered solution of $pH\ 8$, then how much material will exist in each of the three forms ${H}_{2}{CO}_{3},H{CO}_{3}^{-}$ and ${CO}_{3}^{2-}$? <div>For ${H}_{2}{CO}_{3}$, ${K}_{1}=5\times {10}^{-7}$; ${K}_{2}=5\times {10}^{-13}$</div>

Question 19 : The ionization constant of benzoic acid is $6.46 \times 10^{-5}$ and $K_{sp}$ for silver benzoate is $2.5\times 10^{-13}$. How many times is silver benzoate more soluble in a buffer of $pH = 3.19$ compared to its solubility in pure water?

Question 20 : In a mixture of a weak acid and its salt, the ratio of the concentration of acid to salt is increased ten-fold. The pH of the solution:

Question 21 : Which of the following mixtures will be a buffer solution when dissolved in $500.00\ ml$ of water?

Question 22 : The solubility of $AgCN$ in a buffer solution of $pH=3$ is: [Given ${K}_{sp}$ of $AgCN=1.2\times {10}^{-6}$ and ${K}_{a}$ for $HCN=4.8\times {10}^{-10}$. Assume that no cyano complex is formed.]

Question 23 : When a solution of silver nitrate is added to pure carbon tetrachloride :

Question 24 : The pH of saturated aqueous solution of $NaClO_4$ is 10. If the K$_{sp}$ of BaOH$_2$ is $5 \times 10^{-13}$, the concentration of $Ba^{2+}$ ions in the solution is:

Question 26 : The work done in which of the following process is equal to the internal energy of the system?

Question 27 : The following data show the change in internal energy of a gas, the heat transferred (into if positive) for a gas, and the work done by a gas as it goes through different processes. Which of the following is an adiabatic process?

Question 28 : In a given process on an ideal gas $dW = 0$ and $dQ < 0$, then for the gas :

Question 29 : For which of the following processes is the relation $dQ=dU$ true ?

Question 30 : A thermos bottle containing coffee is vigorously shaken. If the coffee is considered as a system, then the temperature of the coffee will :

Question 31 : The increase in volume of air, when temperature of 600 ml of it, is increased from $27^oC$ to $47^oC$ under constant pressure, is

Question 33 : If an ideal gas, at constant temperature and pressure, expands, then its

Question 34 : A monatomic gas is compressed adiabatically to $\dfrac { 1 }{ 4 }^{ th }$ of its original volume, the final pressure of gas in terms of initial pressure P is:

Question 35 : In an isochoric process if $T_{1}$ = $27^{\circ}$C, then $P_{1}/P_{2}$ will be equal to

Question 36 : Define mixtures. (a) $H_2(g) + \dfrac{1}{2} O_2(g) \rightarrow H_2 O(l)$; $\Delta H^o_{298\ K}= - 285.9\ kJ mol^{-1}$ (b) $H_2(g) + \dfrac{1}{2}O_2(g) \rightarrow H_2O(g)$; $\Delta H^o_{298\ K} = -241.8\ kJ mol^{-1}$ The molar enthalpy of vapourisation of water will be:

Question 37 : How many calories are needed to heat 100g of water from 278K to 288K ?

Question 38 : Equation of first law of thermodynamics for an isochoric process is

Question 39 : A gas is expanded from volume $V_{0}$ to $2V_{0}$ under three different processes. Process 1 is isobaric process, process 2 is isothermal and process 3 is adiabatic. Let $\Delta U_{1},\Delta U_{2}$ and $\Delta U_{3}$ be the change in internal energy of the gas in these three process. Then

Question 40 : The enthalpy of fusion of ice is $6.02  kJ  mol^{ -1 }$. The heat capacity of water is $4.18  J  g^{ -1 }C^{ -1 }$. What is the smallest number of ice cubes at $0^{ \circ }C$, each containing one mole of  water, that are needed to cool $500  g$ of liquid water from $20^{ \circ }C$ to $0^{ \circ }C$.

Question 41 : Find the change in the internal energy when 15 gm of air is heated from $0^{o}C$ to $5^{o}C$. The specific heat of air at constant volume is 0.2 cal/gm$^{o}C$.

Question 43 : For an adiabatic expansion of a mono atomic perfect gas, the volume increase by 24%. What is the percentage decrease in pressure?

Question 44 : In which of thee following processes, heat is neither absorbed nor released by a system ?

Question 45 : Assertion: The heat of vaporization of water and the heat of fusion of water is numerically different. Reason: When water freezes or vaporizes, its chemical composition remains unchanged.

Question 46 : An athlete is given $100  g$ of glucose $(C_6H_{ 12 }O_6)$ of energy equivalent to $1560  kJ$. He utilises $50 \%$ of this gained energy in the event. In order to avoid storage of energy in the body, calculate the weight of water he would need to perspire. The enthalpy of evaporation of water is $44  kJ/ mol$

Question 47 : ${H}_{2}(g)+\cfrac { 1 }{ 2 } { O }_{ 2 }(g)\rightarrow {H}_{2}O(g);\Delta H=x$ ${H}_{2}(g)+\cfrac { 1 }{ 2 } { O }_{ 2 }(g)\rightarrow {H}_{2}O(l);\Delta H=y$ Heat of vaporisation of water is:

Question 48 : Statement 1: $320$ calories or $1.34\times 10^{3}$ joules of heat will melt $4$ grams of ice at $0^o$C. Statement 2: The heat of fusion of water is $80$ calories per gram or $3.34\times 10^2$ joules per gram.

Question 49 : Root mean square velocity of molecules of a diatomic gas is to be increased to 1.5 times, If the process is done adiabtically, the ratio of initial volume to the final volumes is :

Question 50 : The temperature of $5\:mol$ of a gas which was held at constant volume was changed from $100^\circ C$ to $120^\circ C$. The change in internal energy was found to be $80\:J$. The total heat capacity of the gas at constant volume will be equal to

Question 51 : The latent heatsof fusion in $Jg^{-1}$ of five substances a (mol.mass =18); b(mol.mass =20); c(mol.mass =30), d(mol.mass =60) and e(mol.mass =30) are respectively $80,45,90,45,45$. Which of the following pair has same value of $\Delta H_{fusion}$?

Question 52 : 5 moles of hydrogen $\left ( \gamma =\dfrac{7}{5}\right )$ initially at S.T.P is compressed adiabatically so that its temperature becomes $400^{o}C$.The increase in internal energy in kilojoules is (R $=$ 8.30 J/mole-K)

Question 53 : A solid object is placed in water contained in an adiabatic container for some time. The temperature of water falls during the period and there is no appreciable change in the shape of the object. The temperature of the solid object

Question 54 : The work done during the expression of gas from $4 dm^3$ to $6 dm^3$ against a constant external pressure of 3 atm is: (1 L atm = 101.32J).

Question 55 : An ideal diatomic gas is heated at constant pressure. What fraction of heat energy is utilized to increase its internal energy?

Question 56 : The normal boiling point of toluene is $110.7^oC$ and its boiling point elevation constant is 3.32 K kg $mol^{-1}$. The enthalpy of vaporization of toluene is nearly:

Question 57 : Consider the following reaction : $CO_{(g)} + \dfrac{1}{2}O_{2(g)} \rightarrow CO_{2(g)}$ <div>How are $\Delta E$ and $\Delta H$ related for the reaction?</div>

Question 58 : The polymerization of ethylene to linear polyethylene is represented by the reaction, $n(CH_2==CH_2)\longrightarrow --(--CH_2--CH_2--)-- _n$ <div>where n has large integral value. Given that the average enthalpies of bond dissociation for $C==C$ and $C--C$ at $298 K$ are $+590$ and $+331 kJ mol^{ -1 }$ respectively. <div> </div><div>Calculate the enthalpy of polymerization per mole of ethylene at $298 K$: </div></div>

Question 59 : An ideal gas at $27^{o} C$ is compressed adiabatically to $\dfrac{8}{27}$ of its original volume. If $\gamma = \dfrac{5}{3}$ , then the rise in temperature is 

Question 60 : A monoatomic gas $(y = 5 / 3)$ us suddenly compressed to $\dfrac{1}{8}$ of its original volume adiabatically, then the pressure of the gas will change to 

Question 61 : Calculate the $\Delta H$ for conversion of C (diamond) to C (graphite) when the following reactions are given: $C(diamond)+O_2 \rightarrow CO_2(g); \: \Delta H = -94.5 \: Kcal$ $C(graphite)+O_2 \rightarrow CO_2(g); \: \Delta H = -94 \: Kcal$

Question 62 : For combustion of $1$ mole of benzene at $25^{\circ} C$ the heat of reaction at constant pressure is $- 780.9$ kcal. What will be the heat of reaction at constant volume? <div>$C_{6}H_{6(l)} + 7 \dfrac{1}{2}O_{2(g)} \rightarrow 6CO_{2(g)} + 3H_{2}O_{(l)}$ </div>

Question 63 : The heat change $\Delta H$ for the reaction $2CO+O_{2}\rightarrow 2CO_{2};\Delta H =-135kcal$ is called?

Question 64 : Two moles of helium gas $(\gamma =5/3)$ are initially at a temperature of $27^o$C and occupy a volume of $20$ litres. The gas is first expanded at constant pressure until the volume is doubled. It then undergoes an adiabatic change until the temperature returns to its initial value. What are the final volume and pressure of the gas?

Question 65 : The pressure and density of a diatomic gas $( \gamma = 7 / 5)$ change adiabatically from (P, d) to (p, d). If $\dfrac{d'}{d} = 32$ then $\dfrac{P'}{P}$ Should be

Question 66 : For free expansion of a gas in an adiabatic container which of the following is true?

Question 67 : Calculate $\Delta U$ if $2 kJ$ heat is released and $10 kJ$ work is done on the system. 

Question 68 : (i) Cis-2-butene $ \rightarrow$ trans-2-butene, $ \Delta H_{1}$ (ii) Cis-2-butene $ \rightarrow$ 1-butene, $ \Delta H_{2}$ (iii) Trans-2-butene is more stable than cis-2-butene. (iv) Enthalpy of combustion of 1- butene, $\Delta H=-647.0 kCal/mol.$ The value of $ \Delta H_{1}$ & $\Delta H_{2}$ respectively in K Cal/mole are

Question 69 : Calculate $\Delta H$ for $C_{(graphite)}\rightarrow C_{diamond}$ from the following data:i) $ C(graphite)+O_{2}\rightarrow CO_{2}(g),\Delta H=-94\:Kcal$ii) $ C(diamond)+O_{2}\rightarrow CO_{2}(g),\Delta H=-68\:Kcal$

Question 70 : An ideal gas is allowed to expand freely against vacuum in a rigid insulated container. The gas undergoes

Question 71 : One mole of an ideal gas at an initial temperature of T K does 6 R joules of work adiabatically. If ratio of specific heats of this gas at constant pressure and at constant volume is 5/3, the final temperature of gas will be

Question 72 : With what minimum pressure  (in $kPa$) a given volume of an ideal gas  $\left( C _ { p , m } = 7 / 2 R \right),$  originally at  $400\ K$  and  $100\ kPa$  pressure can be compressed irreversibly adiabatically in order to raise its temperature to  $600\ K$  :

Question 74 : $\Delta _fH$ of graphite is 0.23 kJ/mol and $\Delta _fH$ of diamond is 1.896 kJ/mol. $\Delta H_{transition}$ from graphite to diamond is :

Question 75 : The polymerisation of ethylene to linear polyethylene is represented by the reaction $\displaystyle nCH_{2}=CH_{2}\rightarrow \left ( -CH_{2}-CH_{2}- \right )n$ where n has a large integral value. Given that average enthalpies of bond dissociation for $\displaystyle C=C$ & $\displaystyle C-C$ at 298 K are $\displaystyle +$ 590 & $\displaystyle +$ 331 kJ $\displaystyle mol^{-1}$ respectively. Then the enthalpy of polymerisation per mole of ethylene at 298 K is:

Question 76 : An ideal gas having initial pressure P, volume V and temperature T is allowed to expand adiabatically until its volume becomes $5.66$V while its temperature falls to $T/2$. Obtain the work done by the gas during the expansion as a function of initial pressure P and volume V.

Question 77 : A gas consisting of rigid diatomic molecules is expanded adiabatically. How many times has the gas to be expanded to reduce the r.m.s. velocity of the molecules to $\left( \frac { 2 } { 3 } \right)$ rd of initial value.

Question 78 : During an isothermal expansion, a confied ideal gas does -150J of work against its surroundings. This implies that

Question 79 : Two litre of $N_2$ at $0^oC$ and 5 atm are expanded isothermally against a constant external pressure of 1 atm until the pressure of gas reaches 1 atm. Assuming the gas to be ideal calculate work of expansion?

Question 80 : The heat of combustion of yellow phosphorous is $-9.9\ kJ$ and of red phosphorous is $-8.78\ kJ$. The heat of transition of yellow phosphorus to red phosphorus is:

Question 81 : What is the enthalpy of vaporisation of liquid water in $kJ \:mol^{-1}$ if:<div> ( i ) $H_2( g ) +\cfrac{1}{2}O_2( g )\longrightarrow H_2O(l)+ 285.77 \:kJmol^{-1}$ ( ii ) $H_2( g ) +\cfrac{1}{2}O_2( g )\longrightarrow H_2O(v)+ 241.84\:kJ \:mol^{-1}$ </div>

Question 83 : From the following data, determine heat of formation ${\Delta _f}{H^0}$ for diborane, ${B_2}{H_{6\left( g \right)}}$ at $298K$ ${B_2}{H_{6\left( g \right)}} + 3{O_{2\left( g \right)}}\rightarrow {B_2}{O_{3\left( s \right)}} + 3{H_2}{O_{\left( g \right)}}\,\,\,\Delta {H_f^0} = - 1941kJ\,mo{l^{ - 1}}$ given ; $\Delta H_f(B_2O_3,solid) = -1273kJ/mol$; $\Delta H_f(H_2O,gas) = -241.8kJ/mol$

Question 84 : A gas is enclosed in a cylinder with a movable frictionless piston. Its initial thermodynamic state at pressure $P_i=10^5$ Pa and volume $V_i=10^{-3}m^3$ changes to a final state at $P_f=(1/32)\times 10^5$ Pa and $V_f=8\times 10^{-3}m^3$ in an adiabatic quasi-static process, such that $P^3V^5=$ constant. Consider another thermodynamic process that brings the system from the same initial state to the same final state in two steps: an isobaric expansion at $P_i$ followed by an isochoric (isovolumetric) process at volume $V_f$. The amount of heat supplied to the system in the two-step process is approximately.

Question 85 : A gas is suddenly compressed to $\frac{1}{4}$ th of its original volume. What is the rise in the temperature, the original temperature being $27^{0}C$ and y = 1.5?

Question 86 : Iron is extracted from iron oxide using carbon monoxide as shown. iron oxide + carbon monoxide $\rightarrow$ iron + carbon dioxide Which statement is correct?

Question 89 : In which of the following reactions, does a non-metal act as a reducing agent?

Question 90 : When Carbon monoxide is passed over heated copper oxide it gives :

Question 91 : Out of the halogens, which one is the most powerful oxidizing agent?

Question 92 : How many moles of electrons are involved in the reduction of one mole of $MnO^-_4$ ion in alkaline medium to $MnO^-_3$?

Question 94 : Electrolysis of water to form hydrogen and oxygen gases is :

Question 95 : Thiosulphate reacts differently with iodine and bromine in the reaction given below. $2S_2O_3^{2-}+I_2 \rightarrow S_4O_6^{2-}+2I^-$ $S_2O_3^{2-}+2Br_2+5H_2O \rightarrow 2SO_4^{2-}+2Br^-+10H^+$ Which of the following statement justifies the above dual behaviour of thiosulphate?

Question 97 : When Magnesium is burnt in air, a white ash remain as left over. What is this?

Question 98 : In the reaction $2Ag\, +\, 2H_2SO_4\, \rightarrow\, Ag_2SO_4 \,+\, 2H_2O\, +\, SO_2$, sulphuric acid acts as :

Question 101 : A certain amount of a reducing agent reduces x mole of $ KMnO_{4}$ and y mole of $ K_{2}Cr_{2}O_{7} $ in different experiments in acidic medium. If the change in oxidation state in reducing agent is same in both experiments, $x:y$

Question 102 : Reaction of iron filings with powdered sulfur is a _____ process.

Question 104 : 'a' g $ KHC_2O_4 $ required to reduce 100 mL of 0.02 M $ KMnO_4 $ in acid medium and 'b'  g $ KHC_2O_4 $neutralises 100 mL of 0.05 $ M Ca(OH)_2 $ then 

Question 105 : The process of black and white photography depends upon the following reaction which is initiated by light. <div>$2Ag^+ + 2Br^-\rightarrow 2Ag + Br_2$ Which of the following species is reduced in this reaction? </div>

Question 107 : Three cations $A, B, C$ are allowed to react with ammonium hydroxide solution. $A$ and $B$ produce a dirty green precipitate and a reddish brown precipitate respectively, both of which do not dissolve on further addition of ${NH}_{4}OH$. $C$ gives pale blue colour precipitate with less amount of ammonium hydroxide and on further addition of ${NH}_{4}OH$, precipitate becomes soluble and deep blue colour solution is formed:

Question 108 : Chemical reactions such as redox reactions involve transfer of ___________one species to other species.

Question 109 : On the basis of the following ${E}^{o}$ values, the strongest oxidising agent is: ${ \left[ Fe{ \left( CN \right)  }_{ 6 } \right]  }^{ 4- }\longrightarrow { \left[ Fe{ \left( CN \right)  }_{ 6 } \right]  }^{ 3+ }+{ e }^{ - },{ E }^{ o }=-0.35V$ ${Fe}^{2+}\rightarrow {Fe}^{3+}+{e}^{-1}$; ${Fe}^{2+}\rightarrow {Fe}^{3+}+{e}^{-1};{E}^{o}=-0.77V$

Question 110 : A dilute Ferrous sulphate solution was gradually added to the beaker containing acidified permanganate solution. The light purple colour of the solution fades and finally disappears. Which of the following is the correct explanation for the observation?

Question 111 : $Al + MnO_4^- \rightarrow Al(OH)_4^- + MnO_2$ For this reaction the oxidation state of $Al$ and $Mn$ in the product are respectively:

Question 112 : Hydrogen sulphide $(H_2S)$ is a strong reducing agent. Which of the following reactions shows its reducing action?

Question 113 : $Al + NO_2^- \rightarrow Al(OH)_4^- + NH_3 $ The oxidizing agent for this reaction is________.

Question 116 : Fill in the blanks by picking the option with appropriate words.  Oxidising agent is a substance which P itself and Q the other. Reducing agent is a substance which R itself and S the other. The reactions which involve be oxidation and reduction are called T reactions.

Question 118 : Which one of the following undergoes reduction with $H_2O_2$ in an alkaline medium?

Question 119 : The number of electrons involved when 1 mole of $H_2O_2$decomposes as $H_2O_2 \longrightarrow H_2O + O_2$ is?

Question 121 : A migration of hydrogen with a pair of electrons is called:

Question 122 : In reaction  $B_2H_6 +2KOH +2X \to 2Y +6H_2$. $X$ and $Y$ are respectively:

Question 123 : Identify the correct statement with respect to the following reaction. $2K_2MnO_4 + Cl_2 \rightarrow 2KCl + 2 KMnO_4$

Question 125 : Dichloroacetic acid $ (CHCl_{2}CO_{2}H) $ is oxidized to $ CO_{2}, H_{2}O $ and $ Cl_{2} $ by 1.2 equivalents of an oxidizing agent. Same amount of the acid can neutralize 'X' moles of $ NH_{2} $ to give ammonium dichloroacetate. $ 'X' $ is 

Question 127 : Statement I: When $O_{3}$ reacts with $KI,O_{3}$ is reduced into $O_{2}$. Statement II: There is no change in oxidation state of oxygen, in this reaction.

Question 128 : In an experiment, 4 g of $M_2O_x$ oxide was reduced to $2.8\ g$ of the metal. If the atomic mass of the metal is $56\, g\, mol^{-1}$. The number of $O-$atoms in the oxide is:

Question 131 : Which of the following given reactions is not a redox reaction?

Question 133 : Which one of the following reactions is an example of redox reaction ?

Question 135 : In acid medium, the standard reduction potential of $NO$ converted to ${ N }_{ 2 }O$ is $1.59 V$. Its standard potential in alkaline medium would be:

Question 137 : According to the Avogadro's Law, equal volumes of two different gases, under same conditions of temperature and pressure, contain equal number of:

Question 140 : The base unit for the length in metric system is :

Question 146 : Equal volume of gases contain equal number of moles.<div>State whether the above statement is true or false.</div>

Question 152 : If the temperature of a water bath is $104^{0}\ F$ then its value in degree Celsius scale will be?

Question 156 : Match the following combinations of electrical units with their terms as single unit: <table class="wysiwyg-table"><tbody><tr><td>Electrical unit</td><td>Single unit</td></tr><tr><td>(I) ampere-second</td><td>A. coulomb</td></tr><tr><td>(II) volt-ampere</td><td>B. ohm</td></tr><tr><td>(III) volt-ampere$^{-1}$</td><td>C. ampere</td></tr><tr><td>(IV) walt/ampere ohm</td><td>D. watt</td></tr><tr><td>(V) joule / ampere second</td><td>E. volt</td></tr></tbody></table>

Question 158 : Find the ratio of boiling point of water and melting point of water in Celsius scale.

Question 160 : The fundamental units in S.I. system, are the same as that of :

Question 163 : Which of the following relations for expressing the volume of a sample is not correct?

Question 166 : Statement 1: $-273^0C$ is also known as absolute zero. Statement 2: $^0C = K + 273 $.

Question 167 : Find the ratio of the boiling point of water and melting point of water in Kelvin scale (up to three decimal places).

Question 173 : Few quantities with their units are listed below. Mark the units which are not correctly matched. (i) Density : kg $m^{-3}$  (ii) Velocity of light : m $s^{-1}$ (iii) Planck's constant : $J^{-1} s^{-1}$ (iv) Acceleration : m $s^{-2}$ (v) Force : kg m

Question 174 : A 5% solution of sugarcane (mol.wt.$=342$) is isotoinc with $1$% solution of $X$ under similar conditions. The mol.wt of $X$ is

Question 176 : Which of the following can be expressed as grams per milliliter?

Question 178 : A solution of hydrochloric acid is required for an experiment. The experimenter must first prepare the solution for use by diluting $10.0 mL$ of the hydrochloric acid to create $200 mL$ of the solution. Which of the following would be the poorest choice of glassware for measuring the solute for the dilution?

Question 180 : Ramu wants to convert the following temperatures from $^oC$ to K. -24, -17, 32, 143. Then the correct increasing order of the above temperatures as per the kelvin scale is

Question 181 : Which one of the following is not a unit of energy?

Question 183 : The difference in temperature of a body measured by $ 27^{\circ}C $. Its corresponding difference is Kelvin scale is?

Question 186 : Match the physical property (in List I) with unit (in List II) :<div> </div><div> <table class="wysiwyg-table"><tbody><tr><td>List-I</td><td>List-II</td></tr><tr><td>a) Viscosity</td><td>i) Jm$^{-2}$</td></tr><tr><td>b) Surface tension</td><td>ii) Nm$^{-1}$</td></tr><tr><td>c) Surface energy</td><td>iii) Kg m$^{-1}$ s$^{-1}$</td></tr><tr><td>d) Vapour pressure</td><td>iv) atm</td></tr></tbody></table></div>

Question 187 : Statement 1: At the same temperature and pressure, 1 L of hydrogen gas and 1 L of neon gas have the same mass. Statement 2: Equal volumes of ideal gases at the same temperature and pressure contain the same number of moles.

Question 188 : Which units of pressure are needed if you are going to use 0.0821 as your ideal gas constant?

Question 189 : What will be the unit of time in that system in which unit of length is m, unit of mass is kg and unit of force is kg wt ?

Question 190 : The unit of rate constant for the reaction, $ 2H_2 + 2NO \rightarrow 2H_2 O  +N_2 $ Which has rate  =  $ k [H_2][NO]^2$ is

Question 192 : If you are driving 55.0 miles per hour, what is your speed in meters per second? <div> </div><div>(1 mile = 1,600 meters)</div>

Question 193 : The density of mercury is 13.6 g/mL. What is the volume of a 200 gram sample of mercury?

Question 194 : In a compound A containing carbon, hydrogen and oxygen, the $\%$ of hydrogen is one sixth that of carbon which is 1.5 times of oxygen. What is the simplest formula for the compound:-

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