9 The Haber process is a reversible reaction. N2(g) + 3H2(g) 2NH3(g) The reaction has a 30% yield of ammonia. Which volume of ammonia gas, NH3, measured at room temperature and pressure, is obtained by reacting 0.75 moles of hydrogen with excess nitrogen?

 3.36 L of ammonia gas

Explanation:

The balanced chemical reaction is:

According to stoichiometry :

3 moles of produce = 2 moles of

Thus 0.75 moles of will producee=  of

But as percent yield is 30 %, amount of ammonia produced =

According to ideal gas equation:

P = pressure  = 1 atm

V = Volume  = ?

n = number of moles = 0.15

R = gas constant =

T =temperature =

Thus 3.36 L of ammonia gas is obtained by reacting 0.75 moles of hydrogen with excess nitrogen.

b is the correct