Ammonia and oxygen react at high temperature | vedclass

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

Question

(A) For the reaction $4 NH_{3(g)} + 5 O_{2(g)} \rightarrow 4 NO_{(g)} + 6 H_2O_{(g)}$,the rate expression is given by: $-\frac{1}{4} \frac{d[NH_3]}{dt

Vedclass · Accepted Answer

$5.4 	imes 10^{-3} \ mol \ L^{-1} \ sec^{-1}$

Vedclass · Answer

(A) For the reaction $4 NH_{3(g)} + 5 O_{2(g)} ightarrow 4 NO_{(g)} + 6 H_2O_{(g)}$,the rate expression is given by: $-\frac{1}{4} \frac{d[NH_3]}{dt} = -\frac{1}{5} \frac{d[O_2]}{dt} = +\frac{1}{4} \frac{d[NO]}{dt} = +\frac{1}{6} \frac{d[H_2O]}{dt}$ Given that the rate of formation of $NO$ is $\frac{d[NO]}{dt} = 3.6 	imes 10^{-3} \ mol \ L^{-1} \ sec^{-1}$. Equating the terms for $NO$ and $H_2O$: $\frac{1}{4} \frac{d[NO]}{dt} = \frac{1}{6} \frac{d[H_2O]}{dt}$ $\frac{d[H_2O]}{dt} = \frac{6}{4} 	imes \frac{d[NO]}{dt} = 1.5 	imes 3.6 	imes 10^{-3} \ mol \ L^{-1} \ sec^{-1}$ $= 5.4 	imes 10^{-3} \ mol \ L^{-1} \ sec^{-1}$

Ammonia and oxygen react at high temperature as in the reaction,$4 NH_{3(g)} + 5 O_{2(g)} \rightarrow 4 NO_{(g)} + 6 H_2O_{(g)}$. If the rate of formation of $NO$ is $3.6 \times 10^{-3} \ mol \ L^{-1} \ sec^{-1}$,calculate the rate of formation of water.

Similar Questions

Write the rate equation for the following reactions:
$1.$ $5 Br^{-}_{(aq)} + BrO^{-}_{3_{(aq)}} + 6 H^{+}_{(aq)} \rightarrow 3 Br_{2_{(aq)}} + 3 H_2O_{(l)}$
$2.$ $R \rightarrow P$
$3.$ $C_4H_9Cl + H_2O \rightarrow C_4H_9OH + HCl$

In a reaction,$n_1 A + n_2 B \rightarrow m_1 C + m_2 D$,$5 \ M$ solution of reactant $A$ is allowed to react with $3 \ M$ solution of reactant $B$. After $5 \ s$,the concentration of $A$ was found to be $4 \ M$. The rate of decomposition of $A$ and the rate of formation of $D$ are respectively $:-$

For the reaction $N_2 + 3H_2 \to 2NH_3$,if $\frac{\Delta [NH_3]}{\Delta t} = 2 \times 10^{-4} \ mol \ L^{-1} s^{-1}$,the value of $\frac{-\Delta [H_2]}{\Delta t}$ would be

For a reaction $\frac{1}{2} A \rightarrow 2 B$,the rate of disappearance of $A$ is related to the rate of appearance of $B$ by the expression:

Find the average rate of formation of $O_{2(g)}$ in the following reaction:
$2 NO_{2(g)} \rightarrow 2 NO_{(g)} + O_{2(g)}$
Given that $\left[-\frac{\Delta[NO_2]}{\Delta t}\right] = x \ mol \ dm^{-3} \ s^{-1}$

Vedclass Test Series

Exam Paper Generator

Online Exam Module