Question 92005ChemistryWAEC

Consider the reaction represented by the following equation: C2H4(g)+3O2(g)→2CO2(g)+2H2O(g)C_2H_4(g) +3O2(g) → 2CO_{2(g)} + 2H_2O_{(g)}. How many moles of ethene would be burnt to produce 1 mole of water?

A

0.05 mole

B

0.10 mole

C

0.20 mole

D

2.00 mole

Step-by-Step Explanation

In the given reaction, one mole of ethene (C2H4C_2H_4) produces two moles of water (H2OH_2O). Therefore, to produce one mole of water, only half a mole of ethene is required. This means that 0.05 moles of ethene will be needed to generate 1 mole of water, based on the stoichiometry of the reaction.

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