8.4g of nitrogen gas is sealed with 5g hydrogen gas in a flask and heated where the following equilibrium is established N2+3H2 [equil]2NH3
At equiilbrium reaction is 60% complete.The gaseous mixture at equilibrium is passed through 500mL 1M HCl solution and cooling the solution crystalizes salt NH4Cl out.
Q1 What mass of NH3 was produced in above reaction?
Q2What mass of ammonium chloride would be formed?
Q3If H2SO4 had been used in place of HCl,what weight of ammonium sulphate would have been crystallized out?
Q4If crystals of ammonium chloride were separated out,molarity of HCl left in the filtrate would be?
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3 Answers
1357N2+3H2→2NH3
moles of N2=2.8/28=0.3
moles of H2=5/2=2.5
here N2 is limiting reactant so reaction will go according to N2
as 60% is complete moles of N2 dissociated=0.18
moles of NH3 formed =2*0.18=0.36
mass of NH3=0.36*17
=6.12 g
1357moles of NH3=0.36
moles of HCl=0.5
moles of NH4Cl formed=0.36
Wt.=0.36*54.5=19.62 g
