For the following reaction, 5.05 grams of potassium hydroxide are mixed with excess potassium hydrogen sulfate. The reaction yields 13.3 grams of potassium sulfate.

Question

For the following reaction, 5.05 grams of potassium hydroxide are mixed with excess potassium hydrogen sulfate. The reaction yields 13.3 grams of potassium sulfate.

KHSO₄ (aq) + KOH (aq)  K₂SO₄ (aq) + H₂O (l)

(1) What is the theoretical yield of potassium sulfate? IN GRAMS

(2) What is the percent yield for this reaction? IN %

Answer 1

You asked the same question 3 times. I'm only going to answer it ONCE.

KHSO₄ (aq) + KOH (aq) ==>  K₂SO₄ (aq) + H₂O (l) ... balanced equation

(1). 5.05 g KOH x 1 mol KOH / 56.1 g x 1 mol K₂SO₄ / mol KOH x 174 g K₂SO₄ / mol = 15.7 g K₂SO₄

(2). % yield = actual yield / theoretical yield (x100%) = 13.3 g / 15.7 g (x100%) = 84.9%