Chemical EquilibriumHard
Question
At 0°C and 1 atm pressure, 1 L of N2O4 decomposes to NO2 according to the equation N2O4(g) $\rightleftharpoons$2NO2 (g). To what extent has the decomposition proceeded when the original volume is 25% less than that of existing volume?
Options
A.0.67
B.0.33
C.0.25
D.0.75
Solution
N2O4 $\rightleftharpoons$ 2NO2
Initial mole a 0
Mole at Equilibrium a – x 2x
From question, $(a + x) \times \frac{75}{100} = a \Rightarrow \alpha = \frac{x}{a} = \frac{1}{3}$
Create a free account to view solution
View Solution FreeMore Chemical Equilibrium Questions
In the following equilibrium N2O4(g) $\rightleftharpoons$2NO2(g), when 5 moles of each is taken and the temperature is k...The equilibrium constant for the reaction w + x ⇋ y + z is 9. If one mole of each of w and x are mixed and there i...The position of equilibrium will shift in the given direction by the addition of inert gas at constant pressure in which...Which of the following hypothetical reactions is favoured by the increase of temperature as well as pressure?...For the system : P(s) ⇋ 2Q(g) + 3 R(g)keeping the temperature constant equilibrium is some how disturbed such that...