In the commercial production of the element arsenic, arsenic (III) oxide is heated with carbon, which reduces the oxide to the metal according to the following
equation:
2As,02 + 3C + 3C0, + 4As
If 8.87 g of As, O, is used in the reaction with excess carbon and 5.21 g of arsenic
is produced, what is the percent yield?

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