Chemical EquilibriumHard
Question
When a mixture of N2 and H2 in the volume ratio of 1: 5 is allowed to react at 700 K and 103 atm pressure, 0.4 mole fraction of NH3 is formed at equilibrium. The value of KP for the below reaction N2(g) + 3H2(g) $\rightleftharpoons$2NH3(g)
Options
A.2.6 × 10–5 atm–2
B.2.6 × 10–4 atm–2
C.2.6 × 103 atm–2
D.5.1 × 10–3 atm–2
Solution
N2(g) + 3H2(g) $\rightleftharpoons$2NH3(g)
Initial moles 1 5 0
Moles at equilibrium 1 – x 5 – 3x 2x
Total moles = (1 – x) + (5 – 3x) + 2x = 6 – 2x
From question, $\frac{2x}{6 - 2x} = 0.4 \Rightarrow x = \frac{6}{7}$
$K_{P} = \frac{(2x)^{2}}{(1 - x) \times (5 - 3x)^{3}} \times \left( \frac{6 - 2x}{P} \right)^{2} = 2.6 \times 10^{- 4}\text{ at}\text{m}^{- 2}$
Create a free account to view solution
View Solution FreeMore Chemical Equilibrium Questions
The equilibrium constant for the reaction: H3BO3 + Glycerin$\rightleftharpoons$ (H3BO3 + Glycerin complex) is 0.90. How ...Consider the following reactions in which all the reactants and products are present in gaseous state$${2xy \rightleftha...A 20 litre container at 400 K contains CO2(g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO)...For the reaction $$\text{CO}(g) + \text{H}_2\text{O}(g) \rightleftharpoons \text{CO}_2(g) + \text{H}_2(g)$$ at a given t...At 0°C and 1 atm pressure, 1 L of N2O4 decomposes to NO2 according to the equation N2O4(g) $\rightleftharpoons$2NO2 (g)....