Ex 2:A reaction of 2.00 g of hydrogen with excess oxygen produced15.8 g of water. What is the yield of this experiment?
Question
Ex 2:A reaction of 2.00 g of hydrogen with excess oxygen produced15.8 g of water. What is the yield of this experiment?
Solution
Step 1: Write down the balanced chemical equation for the reaction.
2H2 + O2 -> 2H2O
Step 2: Calculate the theoretical yield.
From the balanced equation, we can see that 2 moles of hydrogen (H2) react to form 2 moles of water (H2O).
The molar mass of hydrogen (H2) is approximately 2 g/mol. So, 2.00 g of hydrogen is approximately 1 mole.
The molar mass of water (H2O) is approximately 18 g/mol. So, theoretically, 1 mole of hydrogen should produce 1 mole of water, which is 18 g.
Step 3: Calculate the actual yield.
The actual yield is given as 15.8 g of water.
Step 4: Calculate the percent yield.
Percent yield = (actual yield / theoretical yield) * 100%
Percent yield = (15.8 g / 18 g) * 100% = 87.78%
So, the yield of this experiment is 87.78%.
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