For the following reaction (production of ethanol) C2H4 +H2O——>C2H5OH A. How many moles of water will be used to produce 10 mol of C2H5OH

B. If you need to produce 27 mol C2H5OH how many moles of C2H4 will be used?

A: 10 moles of water are required.

B: 27 moles of C₂H₄  are used.

Explanation:

A:

Given data:

Moles of water used = ?

Moles of C₂H₅OH formed = 10 mol

Solution:

Chemical equation:

C₂H₄ + H₂O     →       C₂H₅OH

Now we will compare the moles of water with C₂H₅OH from balance chemical equation:

                    C₂H₅OH            :           H₂O  

                         1                   :             1

                       10                  :         10

10 moles of water are required.

B)

Given data:

Moles of C₂H₄ used = ?

Moles of C₂H₅OH formed = 27 mol

Solution:

Chemical equation:

C₂H₄ + H₂O     →       C₂H₅OH

Now we will compare the moles of C₂H₄  with C₂H₅OH from balance chemical equation:

                    C₂H₅OH         :           C₂H₄  

                         1                 :             1

                         27               :            27

27 moles of C₂H₄  are used.

i think it is true since you can test the answer and can use observations to complete it.

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.