Question

I
Suppose 1.65 moles of C6H6
react with excess oxygen to produce carbon dioxide
and water
a. How many moles of carbon dioxide will be produced in this reaction?
b. How many moles of water will be produced in this reaction?
c.
How many moles of oxygen gas will be consumed during the reaction?
​

Answer 1

Answer:

1 9.9

2 4.95

3 12.375

Explanation:

To solve this problem, we basically need to write a balanced chemical equation:

Like all other hydrocarbons, benzene burns in oxygen to yield water and carbon iv oxide as the only products. A balanced chemical equation is given below:

2C6H6(l)+15O2(g)→12CO2(g)+6H2O(g)

Let’s now proceed to answer the questions.

A. Number of moles of carbon iv oxide produced

From the balanced chemical equation, we can see that one mole of benzene yielded 6 moles of carbon iv oxide.

This means 1.65 moles of benzene will yield: 6 * 1.65 = 9.9 moles of CO2

B. From the balanced equation, we can see that one mole of benzene yielded 3 moles of water. Hence, 1.65 moles will yield 1.65 * 3 = 4.95 moles of water

C. To find the number of moles of oxygen consumed, we can see that 2 moles of benzene consumed 15 moles of oxygen. 1.65 moles of benzene would thus consume 1.65 * 15/2moles = 12.375moles of oxygen

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