Each step in the following process has a yield of 90.0 %. ch 4 + 4 cl 2 ⟶ ccl 4 + 4 hcl ccl 4 + 2 hf ⟶ ccl 2 f 2 + 2 hcl the ccl 4 formed in the first step is used as a reactant in the second step. if 3.00 mol ch 4 reacts, what is the total amount of hcl produced? assume that cl 2 and hf are present in excess.

4.86 moles of HCl

Explanation:

1. First write the balanced chemical equations involved in the process:

2. Calculate what amount of is formed in the first reaction.

As the yield of each reaction is 90.0%, the amount of produced is the following:

3. Calculate the amount of HCl produced.

The total amount of HCl produced with a 90.0% yield is:

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