For the following reaction, 6.81 grams of hydrogen gas are mixed with excess iodine. The reaction yields 743 grams of hydrogen iodide. hydrogen (g) + iodine (s) hydrogen iodide (g) What is the theoretical yield of hydrogen iodide?

percentage yield = 84. 60%

Explanation:

The reaction involved hydrogen and iodine. The chemical equation of the reaction should be balanced before solving the question.

H2 (g) + I2 (g) → HI

The balanced equation

H2 (g) + I2 (g) → 2 HI (g)

molar mass of hydrogen gas = 2 g

molar mass of hydrogen iodide = 2 + 127 = 129 g

2 moles of hydrogen iodide = 2 * 129 = 258 g

2 g of hydrogen gas produces 258 g of hydrogen iodide

6.81 g of hydrogen will produce? gram of hydrogen iodide

theoretical yield of hydrogen iodide = (6.81 * 258) / 2

theoretical yield of hydrogen iodide = 1756.98 / 2

theoretical yield of hydrogen iodide = 878.49 g

percentage yield = actual yield/theoretical yield * 100

percentage yield = 743/878.49 * 100

percentage yield = 74300/878.49

percentage yield = 84.5769445298

percentage yield = 84. 60%