How many grams of $C O_{2}$ formed when 7.0 g of ethene $(C_{2} H_{4})$ burns in oxygen?

$C_{2} H_{4} + 3 O_{2} \to 2 C O_{2} + 2 H_{2} O$

9.0

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22

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44

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82

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180

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Solution

The correct option is B $22$ g
Molar mass of ethene $C_{2} H_{4} = 2 (12) + 4 (1) = 28$ g/mol

7.0 g ethene corresponds to $\frac{7.0 g}{28 g / m o l} = 0.25$ moles
1 mole of ethene gives 2 moles of $C O_{2}$ .

0.25 moles of ethene will give 0.50 moles of $C O_{2}$ .
Molar mass of $C O_{2}$ is 44 g/mol.

Mass of $C O_{2}$ will be $44$ g/mol $\times$ 0.50 mol $=$ $22 g$

Hence, option B is correct.

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