For the reaction 2A_{(g)} + B_{(g)} rightleft | vedclass

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

Question

(C) The given reaction is $2A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + 362 \, kcal$.
Since the reaction is exothermic $(\Delta H < 0)$,accordi

Vedclass · Accepted Answer

$1000 \, atm$ and $50 \, ^\circ C$

Vedclass · Answer

(C) The given reaction is $2A_{(g)} + B_{(g)} ightleftharpoons C_{(g)} + 362 \, kcal$.
Since the reaction is exothermic $(\Delta H < 0)$,according to Le Chatelier's principle,a lower temperature will shift the equilibrium to the right,favoring the formation of products.
For the pressure effect,we look at the change in the number of moles of gas: $\Delta n_g = n_{	ext{products}} - n_{	ext{reactants}} = 1 - (2 + 1) = -2$.
Since $\Delta n_g < 0$,an increase in pressure will shift the equilibrium towards the side with fewer moles of gas,which is the product side.
Therefore,high pressure and low temperature favor the formation of $C$.

For the reaction $2A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + 362 \, kcal$,which combination of pressure and temperature will favor the formation of $C$ at equilibrium?

Similar Questions

Which among the following reactions is favoured in the forward direction by an increase in temperature?

Which of the following changes will not alter the equilibrium concentration of ammonia in the reaction: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} \quad \Delta H = -x \text{ kJ}$?

In a reversible reaction,a catalyst...

When $NaNO_{3(s)}$ is heated in a closed vessel,$O_{2(g)}$ is released and $NaNO_{2(s)}$ remains. The equilibrium is: $NaNO_{3(s)} \rightleftharpoons NaNO_{2(s)} + 1/2 O_{2(g)}$. Which of the following is correct?

$N_2$ and $O_2$ combine to form nitric oxide as follows: ${N_2}_{(g)} + {O_2}_{(g)} \rightleftharpoons 2NO - \text{heat}$. Which of the following conditions will favor the production of $NO$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module