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%

it should be p1 v1 = p2 v2

i'm assuming that it's c.) red bank..