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Consider the balanced chemical equation that follows. You are asked to determine how many moles of water you can produce from 4.0 mol of hydrogen and excess oxygen. (Excess oxygen means that so much oxygen is available it will not run out.) Which of the numbers that appear in the balanced chemical equation below are used to perform this calculation?

2H2(g)+O2(g)→2H2O(l)

A. the coefficients for hydrogen and oxygen are used
B. the coefficients for water and hydrogen are used
C. the subscripts for water and hydrogen are used

Answer :

Ondinne

Answer:

B. The coefficients for water and hydrogen are used.

Explanation:

You have the balanced chemical reaction given by the problem:

[tex]_{2}H_{2}_{(g)}+O_{2}_{(g)}=_{2}H_{2}O_{(l)}[/tex]

If the oxygen is in excess, it means that the hydrogen is the limiting reagent, so, to calculate the number of moles you can produce from 4.0 moles of hydrogen you use the stoichiometric coefficients as follows:

[tex]4.0molesH_{2}*\frac{2molesH_{2}O}{2molesH_{2}}=4.0molesH_{2}O[/tex]

So, the correct answer is B, the coefficients for water and hydrogen are used.

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