Problem: Consider the combustion of H2(g): 2 H2(g) + O2(g) → 2 H2O(g). If hydrogen is burning at the rate of 0.50 mol/s, what is the rate of consumption of oxygen?

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FREE Expert Solution

We can simply do a rate-to-rate comparison based on the stoichiometric coefficients.

Reaction: 2 H2(g) + O2(g) → 2 H2O(g)

Given:

[H2]t=0.50 mols


For O2(g): Since O2 is a reactant, the rate should be negative since reactants are consumed/decreased

The rate with respect to O2 is:

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Problem Details

Consider the combustion of H2(g): 2 H2(g) + O2(g) → 2 H2O(g). If hydrogen is burning at the rate of 0.50 mol/s, what is the rate of consumption of oxygen?

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Our tutors have indicated that to solve this problem you will need to apply the Average Rate of Reaction concept. You can view video lessons to learn Average Rate of Reaction. Or if you need more Average Rate of Reaction practice, you can also practice Average Rate of Reaction practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Ratliff's class at USF.