Question 1 :
Which of the following term is denoted as Formula Mass Unit?
Question 3 :
Two elements $A$ and $B$ contain $13$ and $8$ protons respectively. If the number of neutrons in them happen to be $14$ and $8$ respectively; the formula unit mass for the compound between $A$ and $B$ unit would be:
Question 4 :
How many molecules of ozone can be decomposed by one atom of chlorine?
Question 5 :
The formula which represents the simple ratio of atoms in a compound is called:
Question 6 :
When atoms of one element are combined with atoms of another element, the result is a(n) _________ of a compound.
Question 7 :
In the reaction $2NaOH+H_{3}PO_{4}\rightarrow Na_{2}HPO_{4}+2H_{2}O$, the Equivalent weight of the acid is
Question 11 :
Who was the first scientist to propose that all matter was made of small spheres called atoms?
Question 12 :
Who postulated that matter is made up of very small particles in 430 BC?
Question 15 :
The empirical formula shows the ......... numbers of atoms of each element in a compound. Fill in the blank.
Question 19 :
........... are made up of atoms that are held together by chemical bonds.
Question 20 :
When mass is enclosed in a system and none is allowed in or out, it's _____ will never change.
Question 21 :
The ratio by mass of sulphur and oxygen in $SO_2$ is:
Question 22 :
Who laid the foundation of chemical sciences by establishing two important laws of chemical combination ?
Question 26 :
3 g of salt having molecular weight 30 is dissolved in 250 g of water. The molality of the solution is:
Question 27 :
A balanced chemical equation is in accordance with the law of conservation of masses___________.
Question 29 :
A compound formed by elements X and Y crystallizes in a cubic structure in which the X atoms are at the corners of a cube and the Y atoms are at the face-centres. The formula of the compound is:
Question 30 :
An inorganic compound contains 5.88% of hydrogen and 94.11% oxygen. Find out the empirical formula of the compound and predict the molecular formula. <br/>
Question 31 :
When two gases combine in a chemical reaction, then the volume needed :
Question 33 :
Different samples of water were found to contain hydrogen and oxygen in the ratio of 1 : 8. This shows the law of:<br/>
Question 36 :
Which of the following is not a postulate of Dalton's atomic theory?
Question 37 :
Assertion: One mole of oxygen and one mole of $SO_2$ contains same number of oxygen atoms.
Reason: The amount of oxygen in one mole of $O_2$ is same as that in one mole of $SO_2$.
Question 40 :
If true enter 1, if false enter 0.<br>$12$ g carbon contains the same number of atoms as $32$ g of the sulphur has.
Question 42 :
$a KMnO_4 + b H_2SO_4 + c FeSO_4 \rightarrow K_2SO_4 + MnSO_4 + Fe_2 (SO_4)_3 + H_2O$.<br/>In this unbalanced stoichiometric equation the values of a, b and c respectively are ?
Question 44 : Equal volume of gases contain equal number of moles.<div>State whether the above statement is true or false.</div>
Question 47 :
If 100 ml of a solution contains 10g of ${ H }_{ 2 }{ SO }_{ 4 }$, then normality of the solution is:
Question 48 :
If true enter 1, if false enter 0.<br>A chemical formula of an ionic compound shows the ratio of the number of atoms of each element present in one formula unit.
Question 51 :
What is the mass of a 15 mL sample of mercury, if the density of mercury (liquid) = 13.55 g/cm$^{3}$
Question 53 :
If the percentage of water of crystallization in $MgSO_4.xH_2O$ is $13\%$, then what is the value of $x$?
Question 54 :
10 ml of a compound containing 'N' and 'O' is mixed with 30 ml of $H_{2}$ to produce $H_{2}O$ (l) and 10 ml of $N_{2}$(g). Molecular formula of compound if both reactants reacts completely, is:
Question 55 :
Which of the following statements is/are correct for the reaction given below?<br>$4Fe+3O_2\rightarrow2Fe_2O_3$
Question 56 :
An oxide of metal M has 40% by mass of oxygen. Metal M has atomic mass of 24. The empirical formula of the oxide :
Question 57 :
The volume of a gas in discharge tube is $\displaystyle 1.12\times 10^{-7}\ mL$ at $STP$. Then the number of molecules of gas in the tube is -
Question 58 :
The equation which is balanced and represents the correct product(s) is?
Question 59 : <div>$342$ g of $20\%$ by mass of $Ba(OH)_2$ solution (specific gravity $=0.57$) is reacted with $200$ mL of $2 \:M\: HNO_3$ according to given balanced reaction.</div><div><br/>$Ba(OH)_2 + 2HNO_3\longrightarrow Ba(NO_3)_2 + 2H_2O$<br/></div><br/>The nature of the final solution is :<br/>
Question 60 :
If a compound on analysis was found to contain $C=18.5\%, H=1.55\%, Cl=55.04\%$ and $O=24.81\%$ then its empirical formula
Question 61 :
The molar concentration of $AgN{O}_{3}$ solution if one drop of $AgN{O}_{3}$ measures $0.05$ mL is :
Question 62 :
One mole of chlorine combines with certain mass of a metal giving 111 g of its chloride. The same mass of metal can displace 2 g of hydrogen from an acid. The atomic mass of the metal is :
Question 63 : Given an equation:<div>$CrO^{2-}_4 + S_2O^{2-}_3 + \overset{\circleddash}{O}H \rightarrow [Cr(OH)_4]^{-}+ SO^{2-}_4$ </div><div>What volume of $0.2\ M$ $Na_2CrO_4$ solution is required to just react with $30$ mL of $0.2\ M$ $Na_2S_2O_3$ solution?<br/></div>
Question 64 :
Sulphuric acid is produced when sulphur dioxide reacts with oxygen and water in the presence of a catalyst according to the reaction: ${ 2SO }_{ 2 }(g)+{ O }_{ 2 }(g)+{ 2H }_{ 2 }O(l)\longrightarrow { 2H }_{ 2 }{ SO }_{ 4 }$. If $5.6$ mol of $SO_{ 2 }$ reacts with $4.8$ mol of ${ O }_{ 2 }$ and an excess of water, what is the maximum number of moles of ${ H }_{ 2 }{ SO }_{ 4 }$ that can be obtained?
Question 65 :
Calculate 'm' of all the ions presents in the solution of $A{L_2}{\left( {S{O_4}} \right)_3}$ for $1M$ solution. Given ${d_{solution}} = 2.342gm/mL$
Question 66 :
A certain vitamin extracted from plant sources has carbon and hydrogen in $8:1$ mass ratio. The percentage of oxygen is nearly $7.3$. The compound gave no test for nitrogen or sulphur or any other element. What should be the empirical formula of the compound?
Question 67 :
An organic compound has $C=60\%, H=13.3\%$ and $O=26.7\%$. Its empirical formula will be
Question 68 :
$1.2$ g of $Mg$ is treated with $100$ mL of $1$ M $H_2SO_4$. Molar concentration of the $H_2SO_4$ solution after complete reaction is : <br/>
Question 69 :
In an organic compound of molar mass greater than $100$ containing only $C,\ H$ and $N$, the percentage of $C$ is $6$ times the percentage of $H$ while the sum of the percentages of $C$ and $H$ is $1.5$ times the percentage of $N$. What is the least molar mass?<br>
Question 70 :
A sample of $1.0$ g solid $Fe_{2}O_{3}$ of $80$% purity is dissolved in a moderately concentrated $HCl$ solution which is reduced by $Zn$ dust. The resulting solution required $16.7$ ml of a $0.1$M solution of oxidant. Calculate the number of electrons taken up by the oxidant.<br>
Question 71 :
If $0.50$ mole of monovalent metal (${M}^{+1}$) halide is mixed with $0.2$ mole of a divalent metal (${L}^{-1}$) phosphate, the maximum number of moles of ${M}_{2}{PO}_{4}$ that can be formed is:
Question 72 :
A chemist wants to prepare diborane by the following reaction:<br>$6LiH+{ 8BF }_{ 3 }\longrightarrow { 6LiBF }_{ 4 }+{ B }_{ 2 }{ H }_{ 6 }$<br> He starts with $2.0$ moles each of $LiH$ and ${ BF }_{ 3 }$. How many moles of ${ B }_{ 2 }{ H }_{ 6 }$ can be prepared?
Question 73 :
Equal weights of zinc and iodine react together and the iodine is completely converted to $ZnI_{2}$. What fraction by weight of the original zinc remains unreacted? ($Zn=65,I=127$ g/mol)
Question 74 :
Assuming complete ionisation, the $pH$ of $ 0.1\ M\ HCl$ is $1$ .The molarity of $H_2SO_4$ with the same $pH$ is:
Question 75 :
What mass of $P_4O_{10}$ will be produced by the combustion of 2.0 g fo $P_4$ with 2.0 g of $O_2$?
Question 76 :
Caffeine has a molecular weight of $194$. It contains $28.9$% by mass of nitrogen. Number of atoms of nitrogen in one molecule of it is:
Question 77 :
The heat of neutralization of a strong base and a strong acid is $13.7$ kcal. The heat released when $0.6$ mole HCl solution is added to $0.25$ mole of NaOH is:
Question 78 :
The action of bacteria on meat and fish produces a poisonous compound called cadaverine. As its name and origin imply, it stinks. It is $58.77$% $C$, $13.81$ % $H$ and $27.42$ % $N$. Its molar mass is $102$ g/mol. Determine the molecular formula of cadaverine.
Question 79 : Two substance, $P_{4}$ and $O_{2}$ are allowed to react completely to form mixture of $P_{4}O_{6}$ and $P_{4}O_{10}$ leaving none of the reactants. The composition of final mixture if $P_{4} $ and $O_{2}$ is taken as:<br/>$P_{4} + 3O_{2}\rightarrow P_{4}O_{6}$<br/>$ P_{4} + 5O_{2}\rightarrow P_{4}O_{10}$.<br/><br/><div>(i) If $1$ mole $P_{4}$; $4$ moles of $O_{2}$<br/>(ii) If $3$ moles $P_{4}$; $11$ moles of $O_{2}$<br/>(iii) If $3$ moles $P_{4}$; $13$ moles of $O_{2}$<br/></div>
Question 80 :
The number of moles of $KMnO_4$ required to oxidize one equivalent of $KI$ in the presence of sulfuric acid is:
Question 81 :
When $100$ mL of $0.1\ M$ $KNO_3$, $400$ mL of $0.2\ M$ $HCl$ and $500$ mL of $0.3\ M$ $H_2SO_4$ are mixed, then in the resulting solution :
Question 82 : $ A + B \rightarrow {A}_{3}{B}_{2} $<br/>$ {A}_{3}{B}_{2} + C \rightarrow {A}_{3}{B}_{2}{C}_{2} $<div><br/>The above two reactions are carried out by taking $4$ moles each of $A$ and $B$ and $2$ moles of $C$. Which of the following option(s) is/are correct?</div>
Question 83 : How many moles of lead (II) chloride will be formed from a reaction between $6.5$ g of $PbO$ and $3.2$ g of $HCl$? <div>[Atomic wt. of $Pb=207$ g/mol]</div>
Question 84 :
$10$ mL of $1\ M\ BaCl_2$ solution and $5$ mL of $0.5\ M\ K_2SO_4$ are mixed together to percipitate out $BaSO_4$. The amount of $BaSO_4$ precipated will be :
Question 85 :
10 mL of gaseous organic compound contain C, H and O only was mixed with 100 mL of $O_{2}$ and exploded under identical conditions and then cooled. The volume left after cooling was 90 mL. On treatment with KOH a contraction of 20mL was observed. If vapour density of compound is 23, derive molecular formula of the compound.
Question 86 :
A quantity of $5\ g$ of a crystalline salt when rendered anhydrous lost $1.8\ g$ of water. The formula mass of the anhydrous salt is $160$. The number of molecules of water of crystallization in the salt is _________.
Question 87 :
Assertion: If $30$ mL of $H_2$ and $20$ mL of $O_2$ react to form water, then $5$ mL of $H_2$ is left at the end of the reaction.
Reason: $H_2$ is the limiting reagent.
Question 88 : A solution is prepared by mixing 8.5 g of $CH_2Cl_2$ and 11.95 g of $CHCl_3$. If vapour pressure of $CH_2Cl_2$ and $CHCl_3$ at 298 K are 415 and 200 mmHg respectively, the mole fraction of $CHCl_3$ in vapour form is:<div><br/>[Molar mass of C1=35.5 g $mol^{-1}$] <br/></div>
Question 89 :
Equivalent weight of $CuSO_{4}$ in terms of its molecular weight M in the following reaction is
Question 90 :
A gaseous mixture of $N_2$ and $O_2$ containing $60\%$ by mol $N_2$ is allowed to react with each other according to the following equation:<br>$N_2 + O_2 \rightarrow NO_2$<br>If $92$ g of $NO_2$ is formed, find the mole of $N_2$ present in the mixture.
Question 91 :
Natural water contains about $0.02\%$ $D_2O$ (heavy water). When it is enriched to $20\%$ (by volume), calculate the fraction of weight due to neutrons in 1 mole of sample.
