Reaction Quotient

Q.

For the system A(g) + 2B(g) $\rightleftharpoons$​ C(g), the equilibrium concentrations are (A)

0.06 mole/litre (B) 0.12 mole/litre (C) 0.216 mole/litre. The $K_{eq}$ for the

reaction is

1. 125

2. 250

3. 416

4. 4 x 10^-3

Q. The equilibrium constant $K_c$ for the reaction
$P_4\left(g\right)\rightleftharpoons 2P_2\left(g\right)$
is $1.4$ at ${400}^{\circ }C.$ Suppose that $3$ mole of $P_4\left(g\right)$ and $2$ moles of $P_2\left(g\right)$ are mixed in 2 litre container at ${400}^{\circ }C$. What is the value of reaction quotient $\left(Q_c\right)$?

1. $\frac{3}{2}$
2. $\frac{2}{3}$
3. $1$
4. None of these

Q. what is the difference b/w chemical and ionic equilibrium

Q. 37.The equilibrium constant if for the following reaction at 842^° C is 7.90×10 . What is kp at same temperature 1/2 F2 (g) = F(g) (1) 8.64×1/100000 (2) 8.26×1/10000 (3) 7.90×1/100 (4) 7.56×1/100

Q. The $K_P$ value for the reaction $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$ at $460{}^{o}C$ is 49. If the initial pressure of $H_2$ and $I_2$ is $0.5atm$ respectively, determine the partial pressure of $H_2$ at equilibrium.

1. $0.22atm$
2. $0.11atm$
3. $0.02atm$
4. $0.01atm$

Q. gibbs free energy of reversible reaction at its equilibrium is

Q. The $K_P$ value for the reaction $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$ at $460{}^{o}C$ is 49. If the initial pressure of $H_2$ and $I_2$ is $0.5atm$ respectively, determine the partial pressure of $H_2$ at equilibrium.

1. $0.22atm$
2. $0.11atm$
3. $0.02atm$
4. $0.01atm$

Q. Calculate the work done (in J) when 4.5 g of $H_2{O}_2$ reacts against a pressure of 1 atm at 25C ?
$2H_2{O}_2\left(\ell \right)\to O2\left(g\right)+2H_{2}O\left(\ell \right)$

1. $-1.63\times {10}^2$
2. $4.5\times {10}^2$
3. $3.2\times {10}^2$
4. $-6.1\times {10}^2$

Q. For the equilibrium
$LiCl.3N{H}_3\left(s\right)\rightleftharpoons LiCl.N{H}_3\left(s\right)+2N{H}_3\left(g\right);$
$K_p=9at{m}^2$ at ${37}^{\circ }C.$ A $5L$ vessel contains $0.1$ mole of $LiCl.N{H}_3$. How many moles of $N{H}_3$ should be added to the flask at this temperature to derive the backward reaction for completion?
Use : $R=0.082{\text{atm L mol}}^{-1}{\text{K}}^{-1}$

1. $0.2$
2. $0.59$
3. $0.69$
4. $0.79$

Q. The ester, ethyl acetate is formed by the reaction between ethanol and acetic acid and their equilibrium is represented as:

Q.

At 298 K and 1 atm pressure, the partial pressures in an equilibrium mixture of $N_2{O}_4$ and $N{O}_2$ are 0.7 and 0.3 atmosphere respectively. What will be the partial pressure of $N{O}_2$ when the gases are in equilibrium at 298 K and at a total (equilibrium) pressure of 10 atmospheres?

1. 1.078 atm

2. 2.23 atm

3. 0.77 atm

4. 1.60 atm

Q.

For the reaction $N_2$+ $O_2$ $\leftrightharpoons$2 NO equilibrium constant is $K_c$

Now if we multiply across the given equation by a constant say 3, the new equilibrium constant is ${K_c}^3$(previous equilibrium raised to the power of the constant 3)

1. True

2. False

Q. $N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right);K_C=4$
This reversible reaction is studied graphically as shown in figure. Select correct statements out of I, II and III
(I) Reaction quotient has maximum value at point A.
(II) Reaction proceeds from left to right at a point when,
$\left[N_2{O}_4\right]=\left[N{O}_2\right]=0.1M$.
(III) $K_c=Q$, when point D or F is reached

1. I, II
2. II, III
3. I, III
4. I, II, III

Q.

The equilibrium composition for the reaction is -

$PC{l}_3+C{l}_2\rightleftharpoons PC{l}_5$

0.20 0.10 0.40 mole/litre

If 0.20 mole of $C{l}_2$ is added at same temp. Find equilibrium concentration of $PC{l}_5$ (KC= 20)

1. 1.20 moles

2. 0.56 moles

3. 0.38 moles

4. 0.48 moles

Q. The standard Gibbs energy change at 300 $K$ for the reaction $2A\rightleftharpoons B+C$ is 2494.2 $J$. At a given time, the composition of the reaction mixture is [A] = $\frac{1}{2}$, [B] = 2 and [C] =$\frac{1}{2}$ . The reaction proceeds in the: ($R$=8.314 $J{K}^{-1}mo{l}^{-1},e=2.718$)

1. forward direction because $Q>K_c$
2. reverse direction because $Q>K_c$
3. forward direction because $Q<K_c$
4. reverse direction because $Q<K_c$

Q.

50.0ml of $AgN{O}_3$ solution of 0.05 M is mixed with 50.0ml of 0.01M $KBr{O}_3$ solution. Will the precipitate of $AgBr{O}_3$ be formed?

Given : $K_{sp}$ of $AgBr{O}_3$ = $6.0\times {10}^{-5}$

1. Precipitate formed

2. No precipitate

3. Ready to get precipitate

4. none

Q. why reversible reactions are never complete

Q. Consider the following equilibrium reaction2HI(g) H2 (g)12(g)usThe above equilibrium is established by initiallytaking HI(g) only. If at equilibrium 1 mol each of thespecies is present, then the vapour density ofequilibrium mixture and degree of dissociation atequilibrium are respectively (I-127g/mol

Q. The Reaction Quotient (Q) for the reaction $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$ is given by $Q=\frac{[N{H}_3{]}^2}{\left[N_2\right][H_2{]}^3}$, the reaction will shift in forward direction if :

1. $Q=K_c$
2. $Q<K_c$
3. $Q>K_c$
4. $Q=0$

Q. One mole of $H_{2}O$ and one mole of $CO$ are taken in 10 L vessel and heated to 725 K. At equilibrium, 40% of water (by mass) reacts with $CO$ according to the equation.
$H_{2}O\left(g\right)+CO\left(g\right)\rightleftharpoons H_2\left(g\right)+{CO}_2\left(g\right)$
Calculate the equilibrium constant for the reaction.

Q. explain the relationship between equilibrium constant , reaction quotient and gibbs energy

Q. Two equilibria exist simultaneously in a vessel at ${25}^{\circ }C$
$\begin{array}{ccccc}NO\left(g\right)& +& N{O}_2\left(g\right)& \stackrel{K_{P1}=0.4at{m}^{-1}}{\rightleftharpoons }& N_2{O}_3\left(g\right)\end{array}$
$\begin{array}{ccc}2N{O}_2\left(g\right)& \stackrel{K_{P2}=8at{m}^{-1}}{\rightleftharpoons }& N_2{O}_4\left(g\right)\end{array}$
If initially only $NO$ and $N{O}_2$ are present in a 3:5 mole ratio and the final pressure at equilibrium of $N{O}_2$ at 0.5 atm, then calculate total pressure (in atm) at equilibrium.