Factors Affecting Rate of Reaction

Q.

In a reaction 3A+ $B_2$ $⟶A_3{B}_2$ if 180 atoms of A and 100 molecules of B react then

1) $B_2$ is limiting reagent and 100 molecules of $A_3{B}_2$ will be formed.

2) A is limiting reagent and 60 molecules of $A_3{B}_2$ is formed

3) A is limiting reagent and 180 molecules of $A_3{B}_2$ will be formed

4) B is limiting reactant and 60 molecules of $A_3{B}_2$ will be formed.

Q. 13. When 20 mole of so2 and 15moles of o2 are passed over catalyst 10moles so3 are formed find volume at ntp

Q. 23. find n factor of the following two reactions 1. kclo3 -----> kcl + 3/2 O2, find n factor of Kclo3 2. (NH4)2Cr2 O7 --------> N2 + Cr2O3+ H2O, find n factor of (NH4)2Cr2O7

Q. 34. In A3(g) gives 3A (g) reaction, the intial concentration of A3 is "a"mol L . If x is the degree of dissociation of A3. The total no. Of miles at equilibrium will be

Q. For the reactionA (g) + 2B (g) <----> C (g) + D (g); Kc=10^12. If the initial no of moles of A, B, C and D are 0.5, 1, 0.5 and 3.5 moles respectively in a one litre vessel. What is the equilibrium concentratioN for B? (1) 10^-4 (2) 2 INTO 10^-4 (3) 4 INTO 10^-4 (4) 8 INTO 10^-4

Q. 14. Reaction BaO2(s) -------> BaO(s) + O2(g), delta H =+ve. In equilibrium condition, pressure of O2 depends on A increase mass of BaO2 B increase mass of BaO C increase temperature on equilibrium D increase mass of BaO2 and BaO both

Q. Which of the following pairs of compound illustrate the law of multiple proportions 1 CuO and Cu2O 2 CaC2 and CaSO4

Q. Q-1 why gay lussacs law is not obey when reactants are not gas?

Q. The mass of N2 required to produce 10 g of NH3 from the reaction is N2 + 3H2 → 2NH3

Q.

Which of the following does NOT affect the rate of a chemical reaction?

1. enthalpy of the reaction

2. concentration of reactants

3. temperature

4. surface area

Q. Q 23/30 The values of observed and calculated molecular weightsof silver nitrate are 90 and 170 respectively. The degree ofdissociation of silver nitrate is

Q. 3g of magnesium combine with 2gof oxygen to form magnesium oxide. What is the weight of magnesium oxide that could be formed from 15g of magnesium?

Q. For an exothermic dissolution process, increase in temperature will result in:

1. No change in solubility
2. Increase in solubility
3. Decrease in solubility
4. Cannot be predicted

Q.

Consider the chemical reaction,
$N_2\left(g\right)+3H_2\left(g\right)\to 2N{H}_3\left(g\right)$
The rate of this reaction can be expressed in terms of time derivatives of concentration of $N_2\left(g\right),H_2\left(g\right)orN{H}_3\left(g\right)$. Identify the correct relationship amongst the rate expressions.

1. $Rate=-\frac{d\left[N_2\right]}{dt}=-\frac{1}{3}\frac{d\left[H_2\right]}{dt}=\frac{1}{2}\frac{d\left[N{H}_3\right]}{dt}$

2. $Rate=-\frac{d\left[N_2\right]}{dt}=-3\frac{d\left[H_2\right]}{dt}=2\frac{d\left[N{H}_3\right]}{dt}$

3. $Rate=\frac{d\left[N_2\right]}{dt}=\frac{1}{3}\frac{d\left[H_2\right]}{dt}=\frac{1}{2}\frac{d\left[N{H}_3\right]}{dt}$

4. $Rate=-\frac{d\left[N_2\right]}{dt}=-\frac{d\left[H_2\right]}{dt}=\frac{d\left[N{H}_3\right]}{dt}$

Q. For dissolution of $C{O}_2\left(g\right)$ in $H_{2}O\left(l\right)$
Which of the following statement is correct?

1. Increase in temperature of the solution will will have no effect on solubility of $C{O}_2$
2. On increasing temperature of the solution , solubility of $C{O}_2$ first increases and then stays constant
3. Increase in temperature of the solution will decrease solubility of $C{O}_2$
4. Increase in temperature of the solution will increase solubility of $C{O}_2$

Q. What happens when mwtals react with organic compounds

Q. 51. The mass of FeSO4 required to liberate 44.8L of gaseous product at STP on its heating is FeSO4- Fe2O3 + SO2 + SO3

Q. 166. Consider the half-cell reaction0_2(g) 4H^+ (aq) + 4e^-→ 2H_20By what factor are n, Q, E and Eo changed if all thestoichiometric coefficients are multiplied by thefactor two

Q. Assertion:Coordination no. of both Na^+ and Cl^- in Nacl is 6. Reason:Second coordination no. of Cl^- in the Nacl unit is 12

Q. The scientist "Q" was experimenting to revive a giant called the Mountain. He accidentally dropped a vial of ammonia on the ground. He saw ammonia react with oxygen and produce NO and water.

Let's say the rate of formation of NO is 3.6 x 10^-3 $M{s}^{-1}$

Calculate

• The rate of disappearance of ammonia
• Rate of formation of water

1. 3.6 x 10^-3 $M{s}^{-1}$ and 3.6 x 10^-3 $M{s}^{-1}$
2. 9 x 10^-3 $M{s}^{-1}$ and 5.4 x 10^-3 $M{s}^{-1}$
3. 7.2 x 10^-3 $M{s}^{-1}$ and 3.6 x 10^-3 $M{s}^{-1}$
4. 3.6 x 10^-3 $M{s}^{-1}$ and 5.4 x 10^-3 $M{s}^{-1}$

Q. are gas laws are applicable in equilibrium reaction?

Q. Consider a gaseous reaction $A\left(g\right)+B\left(g\right)\to 3C\left(g\right)$, the rate of the reaction is given by $r=k\left[A\right]{\left[B\right]}^2$. If the volume of the reaction vessel containing these gases is suddenly reduced to $\frac{1}{4}$th of the initial volume, then the rate of the reaction relative to the original rate would be:

1. 64 times
2. 16 times
3. $\frac{64}{3}$ times
4. $\frac{64}{27}$ times

Q.

Consider the chemical reaction,
$N_2\left(g\right)+3H_2\left(g\right)\to 2N{H}_3\left(g\right)$
The rate of this reaction can be expressed in terms of time derivatives of concentration of $N_2\left(g\right),H_2\left(g\right)orN{H}_3\left(g\right)$. Identify the correct relationship amongst the rate expressions.

1. $Rate=-\frac{d\left[N_2\right]}{dt}=-\frac{1}{3}\frac{d\left[H_2\right]}{dt}=\frac{1}{2}\frac{d\left[N{H}_3\right]}{dt}$

2. $Rate=-\frac{d\left[N_2\right]}{dt}=-3\frac{d\left[H_2\right]}{dt}=2\frac{d\left[N{H}_3\right]}{dt}$

3. $Rate=\frac{d\left[N_2\right]}{dt}=\frac{1}{3}\frac{d\left[H_2\right]}{dt}=\frac{1}{2}\frac{d\left[N{H}_3\right]}{dt}$

4. $Rate=-\frac{d\left[N_2\right]}{dt}=-\frac{d\left[H_2\right]}{dt}=\frac{d\left[N{H}_3\right]}{dt}$

Q. How can Gay Lussacs law be applied to volumes of products and reactants in a chemical reaction?

Q. Calculate the volume of SO2 liberated at STP when 15g of Cu reacts with excess concentrated H2SO4
Cu+ 2H2SO4 ------------------- CuSO4 + 2H2O + SO2

Q. 4.5 moles each of hydrogen and iodine heated in a sealed ten litre vessel. At equilibrium, 3 moles of HI were found. The equilibrium constant for ${{\mathrm{H}}_2}_{\left(\mathrm{g}\right)}+{\mathrm{I}}_{2\left(\mathrm{g}\right)}\rightleftharpoons 2{\mathrm{HI}}_{\left(\mathrm{g}\right)}$ is:-
(A) 1 (B) 10 (C) 5 (D) 0.33

Q. the mass of Mercury oxide required to produce 18 gram of oxygen by thermal decomposition

Q. For a reaction $2N_2{O}_5\left(g\right)$$\to 4N{O}_2\left(g\right)+O_2\left(g\right)$ , the rate and rate constant are $1.02\times {10}^{-4}$ $mol{L}^{-1}{s}^{-1}$ and $3.4\times {10}^{-5}{s}^{-1}$ respectively. The concentration of $N_2{O}_5$ at this time will be:

1. 1.732 mol/L
2. 3 mol/L
3. $1.02\times {10}^{-4}$ mol/L
4. $3.2\times {10}^5$ mol/L