1.1 mol of A are mixed with 2.2 mol of B an | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The reaction is $A + 2B \rightleftharpoons 2C + D$. Initial moles: $A = 1.1, B = 2.2, C = 0, D = 0$. At equilibrium,let the concentration of $C$ b

Vedclass · Accepted Answer

$0.001$

Vedclass · Answer

(A) The reaction is $A + 2B ightleftharpoons 2C + D$. Initial moles: $A = 1.1, B = 2.2, C = 0, D = 0$. At equilibrium,let the concentration of $C$ be $0.2 \ M$. Since the volume is $1 \ L$,moles of $C = 0.2$. According to the stoichiometry,if $2 \ mol$ of $C$ are formed,$1 \ mol$ of $A$ is consumed and $2 \ mol$ of $B$ are consumed,and $1 \ mol$ of $D$ is formed. For $0.2 \ mol$ of $C$ formed,$0.1 \ mol$ of $A$ is consumed,$0.2 \ mol$ of $B$ is consumed,and $0.1 \ mol$ of $D$ is formed. Equilibrium moles: $A = 1.1 - 0.1 = 1.0 \ mol$,$B = 2.2 - 0.2 = 2.0 \ mol$,$C = 0.2 \ mol$,$D = 0.1 \ mol$. Equilibrium concentrations: $[A] = 1.0 \ M, [B] = 2.0 \ M, [C] = 0.2 \ M, [D] = 0.1 \ M$. $K_c = \frac{[C]^2 [D]}{[A] [B]^2} = \frac{(0.2)^2 (0.1)}{(1.0) (2.0)^2} = \frac{0.04 	imes 0.1}{1.0 	imes 4} = \frac{0.004}{4} = 0.001$.

Similar Questions

$\Delta n$,the change in the number of moles for the reaction,$C_{12}H_{22}O_{11(s)} + 12O_{2(g)} \rightleftharpoons 12CO_{2(g)} + 11H_2O_{(l)}$ at $25 \ ^\circ C$ is

For the reaction $N_2O_{4_{(g)}} \rightleftharpoons 2NO_{2_{(g)}}$ at $298 \ K$,the equilibrium constant $K_p$ is $0.14 \ atm$. Calculate the value of $K_c$. $(R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$

The equilibrium constant $(K_P)$ for the reaction $2SO_2 + O_2 \rightleftharpoons 2SO_3$ at $1000 \ K$ is $3.5$. The partial pressure of oxygen gas to give equal mole of $SO_2$ and $SO_3$ is $... \ atm$.

The equilibrium constant $K_c$ for the reaction $HA + B \rightleftharpoons BH^{+} + A^{-}$ is $100$. If the rate constant for the forward reaction is $10^5$,then the rate constant for the backward reaction is:

Find the value of $\frac{P}{K_p}$ for the reaction at a certain temperature: $2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$,where $P$ is the total pressure of gases at equilibrium and $P_{Br_2} = \frac{P}{9}$.

Vedclass Test Series

Exam Paper Generator

Online Exam Module