Chemical EquilibriumMedium
Question
Forty percent of a mixture of 0.2 mol of N2 and 0.6 mol of H2 reacts to give NH3 according to the equation
N2(g) + 3H2 (g) $\rightleftharpoons$2NH3(g) at constant temperature and pressure. Then, the ratio of the final volume to the initial volumes of gases is
Options
A.4: 5
B.5: 4
C.7: 10
D.8: 5
Solution
N2 + 3H2 $\rightleftharpoons$ 2NH3
0.2 mole 0.6 mole 0
Equilibrium $0.2 - 0.2 \times \frac{40}{100}$ 0.6 – 0.08 × 3 2 × 0.08
= 0.12 = 0.36 = 0.16
$\therefore\frac{V_{\text{final}}}{V_{\text{initial}}} = \frac{n_{\text{final}}}{n_{\text{initial}}} = \frac{0.64}{0.80} = \frac{4}{5}$
Create a free account to view solution
View Solution FreeMore Chemical Equilibrium Questions
An amount of solid NH4HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm. Pres...The average person can see the red colour imparted by the complex [Fe(SCN)]2+ to an aqueous solution if the concentratio...In the decomposition equilibrium of a certain alkaline earth metal carbonate, the partial pressure of CO2 becomes a hund...For the gas phase reaction 2NO(g) $\rightleftharpoons$N2(g) + O2(g); ΔH = – 43.5 kcal. Which one of the following is tru...The dissociation of ammonium carbamate may be represented by the equation NH4CO2NH2(s) ⇋ 2NH3(g) + CO2(g)ᐃH0...