For the reaction N_{2(g)} + 3H_{2(g)} to 2NH_ | vedclass

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

Question

(C) The rate of reaction $r$ is given by: $r = -\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$.Given the rate of formation of $NH_3$

Vedclass · Accepted Answer

$0.00017 \ kg \ L^{-1} \ h^{-1}$

Vedclass · Answer

(C) The rate of reaction $r$ is given by: $r = -\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$.Given the rate of formation of $NH_3$ is $0.001 \ kg \ L^{-1} \ h^{-1}$.To find the rate of consumption of $H_2$ in terms of mass,we use the stoichiometry: $\frac{d[H_2]}{dt} = \frac{3}{2} 	imes \frac{d[NH_3]}{dt}$.Since the rate is given in $kg \ L^{-1} \ h^{-1}$,we can directly use the stoichiometric coefficients: $	ext{Rate of consumption of } H_2 = \frac{3}{2} 	imes (	ext{Rate of formation of } NH_3) 	imes \frac{M_{H_2}}{M_{NH_3}}$.$M_{H_2} = 2 \ g/mol$ and $M_{NH_3} = 17 \ g/mol$.Rate of consumption of $H_2 = \frac{3}{2} 	imes 0.001 	imes \frac{2}{17} \approx 0.000176 \ kg \ L^{-1} \ h^{-1}$.Rounding to the nearest provided option,the answer is $0.00017 \ kg \ L^{-1} \ h^{-1}$.

For the reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$ under certain conditions of temperature and partial pressure of the reactants,the rate of formation of $NH_3$ is $0.001 \ kg \ L^{-1} \ h^{-1}$. The rate of consumption of $H_2$ under the same condition is $..... \ kg \ L^{-1} \ h^{-1}$.

Similar Questions

The reaction given below $2 NH_{3(g)} \xrightarrow{Pt} N_{2(g)} + 3 H_{2(g)}$ has a rate of reaction of $2.5 \times 10^{-6} \ mol \ dm^{-3} \ sec^{-1}$. What is the rate of formation of $H_{2(g)}$?

For the reaction $2A + B \to A_2B$,the rate of reaction with respect to $A$ is $3.9 \times 10^{-9} \ mol \ L^{-1} \ s^{-1}$. Calculate the rate of consumption of $B$ and the rate of formation of $A_2B$.

Observe the following reaction: $2 A + B \longrightarrow C$. The rate of formation of $C$ is $2.2 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$. What is the value of $-\frac{d[A]}{d t}$ (in $mol \ L^{-1} \ min^{-1}$)?

Explain the relation between the rate of reaction and the stoichiometric coefficients of a balanced chemical equation with examples.

For the reaction $N_2 + 3H_2 \rightarrow 2NH_3$,if $\frac{d[NH_3]}{dt} = 2 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$,then what is the value of $-\frac{d[H_2]}{dt}$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module