Chemical EquilibriumHard
Question
1 mol of N2 is mixed with 3 mol of H2 in a litre container. If 50% of N2 is converted into ammonia by the reaction N2 + 3H2(g) ⇋ 2NH3(g), then the total number of moles of gas at the equilibrium are
Options
A.1.5
B.4.5
C.3.0
D.6.0
Solution
α = 50 % = 
= 0.5
N2 + 3H2 ⇋ 2NH3
Initial 1 3 0
Final 1 - α 3 - 3α 2α
Total moles = 1 - α + 3 - 3α + 2α
= 4 - 2α
= 4 - 2 × 0.5 = 3
= 0.5N2 + 3H2 ⇋ 2NH3
Initial 1 3 0
Final 1 - α 3 - 3α 2α
Total moles = 1 - α + 3 - 3α + 2α
= 4 - 2α
= 4 - 2 × 0.5 = 3
Create a free account to view solution
View Solution FreeMore Chemical Equilibrium Questions
If ‘a’ is the fraction of ammonia present by volume in an equilibrium mixture made from one volume of N2 and three volum...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 NH2COONH4(s) $\rightleftharpoons$2NH3(g) + CO2(g), KP = 3.2 × 10−5 atm3. The total pressure of the gase...When pressure is applied to the equilibrium system Ice$\rightleftharpoons$water, which of the following phenomenon will ...Which of the following hypothetical reactions is favoured by the increase of temperature as well as pressure?...