I NEED WORK SHOWN ON HOW TO GET THE CORRECT ANSWER (WHICH ARE LOCATED IN THE PARENTHESIS) AND ROUNDED TO CORRECT SIG FIGS

3Cl2 + 2N2 → 2N2Cl3

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)