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
Steam reacts with iron at high temperature to give hydrogen gas and Fe3O4(s). The corrent expression for the equilibrium...In a closed container maintained at 1 atm pressure and 25o C, 2 moles of SO2(g) and 1 mole of O2(g) were allowed to reac...When pressure is applied to the equilibrium system Ice$\rightleftharpoons$water, which of the following phenomenon will ...The average person can see the red colour imparted by the complex [Fe(SCN)]2+ to an aqueous solution if the concentratio...A quantity of 60 g of CH3COOH and 46 g of CH3CH2OH reacts in 5 L flask to form 44 g of CH3COOC2H5 at equilibrium. On tak...