For a first-order gas-phase reaction A(g) to | vedclass

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

Question

(A) $1$. Consider the reaction: $A(g) 	o B(g) + C(g)$.$2$. At $t = 0$,the initial pressure of $A$ is $p_i$,and the pressures of $B$ and $C$ are $0$.$

Vedclass · Accepted Answer

$\frac{1}{t} \ln \frac{p_i}{2p_i - p_t}$

Vedclass · Answer

(A) $1$. Consider the reaction: $A(g) 	o B(g) + C(g)$.$2$. At $t = 0$,the initial pressure of $A$ is $p_i$,and the pressures of $B$ and $C$ are $0$.$3$. At time $t$,let $x$ be the decrease in pressure of $A$. The pressures are: $P_A = p_i - x$,$P_B = x$,and $P_C = x$.$4$. The total pressure $p_t$ at time $t$ is given by: $p_t = (p_i - x) + x + x = p_i + x$.$5$. From this,we find $x = p_t - p_i$.$6$. The partial pressure of $A$ at time $t$ is $P_A = p_i - x = p_i - (p_t - p_i) = 2p_i - p_t$.$7$. For a first-order reaction,the rate constant $k$ is given by: $k = \frac{1}{t} \ln \frac{p_i}{P_A}$.$8$. Substituting $P_A$,we get: $k = \frac{1}{t} \ln \frac{p_i}{2p_i - p_t}$.

For a first-order gas-phase reaction $A(g) \to B(g) + C(g)$,let $p_i$ be the initial pressure of gas $A$ and $p_t$ be the total pressure of the reaction mixture at time $t$. The expression for the rate constant $(k)$ is:

Similar Questions

If $50 \%$ of the reactant is converted into a product in a first order reaction in $25 \ min$,how much of it would react in $100 \ min$ (in $\%$)?

If the rate constant of a first order reaction is $4.606 \times 10^{-3} \ s^{-1}$,then find the time required for $400 \ g$ of the reactant to reduce to $50 \ g$. (in $min$)

Identify True $(T)$ and False $(F)$ statements for the following expressions regarding a first-order reaction $R \rightarrow P$:
Statement $I$: $\text{Rate} = -\frac{d[R]}{dt} = k[R]$
Statement $II$: $\text{Rate} = -\frac{d[R]}{dt} = -k[R]$

$A$ first order reaction requires $30 \ min$ for $50\%$ completion. The time required to complete the reaction by $75\%$ will be .......... $\min.$

The rate constant for the decomposition of $H_2O_2$ is $3.66 \times 10^{-3} \ s^{-1}$. If the initial concentration of $H_2O_2$ is $0.882 \ M$,then in how many seconds will its concentration become $0.600 \ M$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module