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)

Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4nh3 (g) + 5o2 (g) → 4no (g) + 6h2o (g) also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition: compound pressure at equilibrium nh3 65.1atm o2 31.3atm no 62.7atm h2o 65.8atm compound pressure at equilibrium nh3 65.3 atm o2 7.79 atm no 12.1 atm h2o 65.8 atm calculate the value of the equilibrium constant kp for this reaction. round your answer to 2 significant