Question 2 :
The substance that initially involved in a chemical reaction is called a reactant.

Question 3 :
A less reactive metal replaces a more reactive metal from its salt solution in water.<br>

Question 4 :
Other signs of a chemical reaction might be an increase in temperature if heat is released or a change in _____.

Question 6 :
Which of the following reaction requires oxygen to be a reactant ?

Question 8 :
Name the type of the following chemical reaction.$2KClO_3 \rightarrow 2KCl +3O_2$

Question 9 :
$FeCl_3 + 3NaOH \rightarrow 3NaCl + Fe(OH)_3$<br/><br/>The reaction is an example of________.

Question 11 :
The chemical equation $Ba{ Cl }_{ 2 }+{ Na }_{ 2 }S{ O }_{ 4 }\rightarrow BaS{ O }_{ 4 }+2NaCl$ represents following type of chemical reaction.

Question 12 :
When hydrogen sulphide gas is passed through a blue solution of copper sulphate, a black precipitate of copper sulphide is obtained and the sulphuric acid so formed remains in the solution. The reaction is an example of:<br/>

Question 13 :
Which substance is serving as a reducing agent in the following reaction?<br/><br/>&#160; &#160; $FeSO_4+Mg\rightarrow MgSO_4+Fe$

Question 15 :
Which of the statements about the reaction below are incorrect ?<br/>$2PbO(s) + C(s) \rightarrow 2Pb(s) + CO_2(g)$<br/><br/>(a) Lead is getting reduced.<br/>(b) Carbon dioxide is getting oxidised.<br/>(c) Carbon is getting oxidised.<br/>(d) Lead oxide is getting reduced

Question 17 :
When sodium sulphate solution reacts with barium chloride solution, the solution after the reaction contains mainly.....

Question 18 :
Assertion: In a reaction<br/><br/>$Z n ( s ) + CuSO_4 (aq) \rightarrow ZnSO_4 (aq) + Cu(s)$<br/><br/>Zn is a reductant but itself get oxidized. Reason: In a redox reaction, oxidant is reduced by accepting electrons and reductant is oxidized by losing electrons.

Question 19 :
For the cell $Zn(s) |Zn^{2+} (aq) || M^{x+} (aq) | M(s)$, different half cells and their standard electrode potentials are given below:<br/><table class="wysiwyg-table"><tbody><tr><td>$M^{x+} (aq/M(s))$</td><td>$Au^{3+} (aq)/Au(s)$</td><td>$Ag^+ \, /Ag(s)$</td><td>$Fe^{3+}(aq)/Fe^{2+} (aq)$</td><td>$Fe^{2+}(aq)/Fe(s)$</td></tr><tr><td>$E^o_{M^{x+}/M^{/(V)}}$<br/></td><td>$1.40$</td><td>$0.80$</td><td>$0.77$</td><td>$-0.44$</td></tr></tbody></table><br/>If $E^o_{Zn^{2+}/Zn} = -0.76 V$, which cathode will give a maximum value of $E^o_{cell}$ per electron transferred ?

Question 20 :
Which of the following chemical reaction is balanced as well as is combustion reaction?

Question 21 :
A quantity of $12\ g$ of magnesium is burnt completely in air $(O_{2}=20\%$ and $N_{2}=80\%$ by volume). Which of the following is/are correct statement(s) regarding this combustion?

Question 23 :
How much $CaO$ is to be added to the furnace charge for each $1280\ kg$ of pure $CaC_{2}$ produced ?

Question 24 :
What is not a mole ratio of $ \displaystyle 6CO_2 + 6H_2O \rightarrow C_6H_{12}O_6 + 6O_2$? <br/>

Question 25 :
We know that balancing of a chemical equation is entirely based on the law of conservation of mass. However the concept of Principle of Atom Conservation (POAC) can also be related to law of conservation of a mass in a chemical reaction. So, POAC can also acts as a technique for balancing a chemical equation. For example, for a reaction&#160;$ABC_3 \rightarrow AB +C_2$&#160;On applying POAC for A, B and C and relating the 3 equation we get : $\dfrac {n_{ABC_3}}{2}=\dfrac {n_{AB}}{2}=\dfrac {n_{C_2}}{3}$ (N= number of moles of X)&#160;Thus the coefficients of $ABC_3$, AB and $C_2$ in the balanced chemical equation will be 2,2 &amp; 3 respectively and the balanced chemical equation can be represented as :$2ABC_3 \rightarrow 2AB +3C_2$Now answer the following question.<br/>&#160;<br/>If the weight ratio of C and $O_2$ present is 1:2 and both of the reactants completely cousumes and form CO and $CO_2$ and we will obtain a gaseous mixture of&#160;CO and $CO_2$&#160;. What would be the weight ratio of CO and $CO_2$&#160; in mixture?

Question 26 :
A metal ($A$) on heating in nitrogen gas gives compound $B$. $B$ on treatment with ${H}_{2}O$ gives a colourless gas which when passed through $Cu{SO}_{4}$ solution gives a dark blue-violet coloured solution. $A$ and $B$ respectively, are :

Question 27 :
What amount of $BaSO_4$ can be obtained on mixing 0.5 mole $BaCl_2$ with 1 mole of $H_2SO_4$ ?

Question 29 :
How many grams of ammonium nitrate will be formed in the reaction?

Question 30 :
A quantity of $6\ g\ NaOH$ and $4.4\ g\ CO_{2}$ is allowed to react to form $Na_{2}CO_{3}$ or $NaHCO_{3}$ or both. Which of the following is correct statement regarding the reaction?

Question 31 :
The reaction, when balanced, $m, n, p$ and $q$ are respectively:<br/>$K_2Cr_2O_7+ \ m FeSO_4+n H_2SO_4\rightarrow Cr_2(SO_4)_3+pFe_2(SO_4)_3+K_2SO_4+qH_2O$&#160;

Question 32 :
An amount of 0.01 mole of $ SO_{2}Cl_{2} $ is hydrolysed completely in sufficientwater (no gas is allowed to escape out ) and the solution is diluted to 200 ml. Which of the following statement is/are correct? (Ag = 108 )

Question 33 :
If the value of $n$ is $2$, then the atomic weight of metal $M$, is

Question 35 :
The equation which is balanced and represents the correct product is:

Question 36 :
Minimum amount of $Ag_2CO_3$ (s) required to produce sufficient amount of oxygen for the complete &#160;combustion of $C_2H_2$ which produces 11.2 L of $CO_2$ at STP after combustion is_________.<br/>$Ag_2CO_3 (s) \, \rightarrow\, 2Ag (s)\, +\, CO_2 (g)\, +\, \dfrac12 O_2 (g)$<br/>$C_2H_2\, +\, \dfrac52 O_2\, \rightarrow\, 2CO_2\, +\, H_2O$<br/>

Question 37 :
A mixture of propane and benzene is burst completely in excess of oxygen at $110^{o}C$. It result the production of equal volumes of $CO_{2}(g)$ and steam (measured under identical pressure and temperature). Which of the following is correct regarding the original mixture?

Question 38 :
What is the minimum mass of ${ CaCO }_{ 3 }(s)$, below which it decomposes completely, required to established equilibrium in a $6.50\ litre$&#160;container for the reaction:<br/>${ CaCO }_{ 3 }(s)\rightleftharpoons CaO(s)+{ CO }_{ 2 }(g);\space { K }_{ c }=0.005\ mole/litre$<br/>