Answer to Question #176044 in General Chemistry for nigel

Question

3Cl

2

 + 2N

2

N2 → 2N

2

Cl

3

Molar masses:

chlorine gas = 70.9 g/mol

nitrogen gas = 28.02 g/mol

dinitrogen trichloride = 134.27 g/mol

a. 1.98 mol of chlorine reacts with 1.98 moles of nitrogen. What is the limiting reactant? (chlorine)

b. What mass of dinitrogen trichloride is produced from the reaction? (177.2364)

c. How many moles of the excess reactant is left over? (0.66)

d. If the percent yield of dinitrogen trichloride is 95.5%, what is the actual yield of the product? (169.2607)

Answer 1

$Moles = \frac{1.98}{70.9}=0.0279$