Consider the combustion of methane in oxygen to produce CO2 and water:                           CH4(g) + O2(g) --> CO2(g) + H2O(g) When methane is being consumed at a rate of 0.65 M/s, what is the rate at which water is being produced?

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Consider the combustion of methane in oxygen to produce CO2 and water:

                          CH4(g) + O2(g) --> CO2(g) + H2O(g)

When methane is being consumed at a rate of 0.65 M/s, what is the rate at which water is being produced?

Expert Solution
Step 1

The rate for a reaction is expressed as :

Chemistry homework question answer, step 1, image 1

Step 2

The reaction given is :

CH4(g) + O2(g) → CO2(g) + H2O(g)

The balanced reaction can be written as :

CH4  (g) + 2 O2  (g) → CO2  (g) + 2 H2O (g)

 

The rate for this reaction can be expressed as :

Chemistry homework question answer, step 2, image 1

Step 3

Given,

Chemistry homework question answer, step 3, image 1

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