Question detail
A balanced chemical equation shows that 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water. If you start with 10 g of hydrogen, calculate the mass of water produced. (Ar of H = 1, Ar of O = 16)
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
Question
Type
exam_style
Style
Topic
Use of amount of substance in relation to masses of pure substances
Question
A balanced chemical equation shows that 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water. If you start with 10 g of hydrogen, calculate the mass of water produced. (Ar of H = 1, Ar of O = 16)
Answer
The mass of water produced is 20 g.
Explanation
This question tests the ability to use a balanced equation to calculate the mass of a product from a given mass of a reactant. It requires understanding of mole ratios and the conversion between mass and moles.
Common mistake
Confusing Ratios
Students often confuse mole ratios with mass ratios when balancing equations, leading to incorrect calculations.
To avoid this mistake, always identify whether you are working with moles or masses and use the correct ratios from the balanced equation.
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