Question

AP Chemistry Algorithmic Question 27

Part A

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:
2Mg(s)+O2(g)→2MgO(s)
When 5.50 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.

Part B

If the percent yield for the following reaction is 75.0%, and 40.0 g of NO2 are consumed in the reaction, how many grams of nitric acid, HNO3(aq) are produced?
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

Part C

Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 9.00 g of oxygen at 25°C. The density of nitrogen monoxide at 25°C is 1.23 g/L.
________ NH3(g) + ________ O2(g) →________ NO(g) + ________ H2O(l)

Answer 1