1.562 g sample of the alcohol CH3CHOHCH2CH3 is burned in an excess of oxygen. What masses of H2O and CO2 should be obtained

Chemistry

1 answer:

eduard [2.5K]28 days ago

7 0

Answer:

$m_{CO_2}=3.709gCO_2 \\\\m_{H_2O}=1.898gH_2O$

Explanation:

Hello.

In this scenario, as the molecular formula for the specified alcohol is C₄H₁₀O (with a molar mass of 74.14 g/mol), its combustion reaction can be represented as follows:

$C_4H_1_0O+6O_2\rightarrow 4CO_2+5H_2O$

This implies a mole ratio of 1:4 with carbon dioxide (molar mass = 44.01 g/mol) and a mole ratio of 1:5 with water (molar mass = 18.02 g/mol), allowing us to determine the resultant masses as follows:

$m_{CO_2}=1.562gC_4H_1_0O*\frac{1mol}{74.14gC_4H_1_0O} *\frac{4molCO_2}{1molC_4H_1_0O} *\frac{44.01gCO_2}{1molCO_2}=3.709gCO_2 \\\\m_{H_2O}=1.562gC_4H_1_0O*\frac{1mol}{74.14gC_4H_1_0O} *\frac{5molH_2O}{1molC_4H_1_0O} *\frac{18.02gH_2O}{1molH_2O}=1.898gH_2O$

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