When a compound containing C and H is burned in oxygen, the reaction produces 0.

Question

When a compound containing C and H is burned in oxygen, the reaction produces 0.90 mol of CO2 and 0.45 mol of H2O.

Determine the number of moles of carbon in the compound. Express your answer using two significant figures.

Determine the number of moles of hydrogen in the compound. Express your answer using two significant figures.

Determine the empirical formula of the compound. Express your answer as a chemical formula.

If one molecule of the compound contains 6 H atoms, what is the molecular formula? Express your answer as a chemical formula.

Write the balanced equation for the combustion reaction. Express your answer as a chemical equation. Identify all of the phases in your answer.

Explanation / Answer

a)

moles of C = moles of CO2 formed

         = 0.90 mol

b)

moles of H = 2*moles of H2O

         = 2*0.45

         = 0.90 mol

c)

there is equal number of C and H

so, empirical formula is CH

d)

molecular formula = C6H6

e)

2C6H6 + 15O2 --> 12CO2 + 6H2O

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