Question

During the analysis, 0.163 g H2O and 0.600 g CO2 are produced. Calcuate the amount (mol) C in the sample, considering the mass of CO2 gas formed by combustion.


0.00905 mol H2O formed

0.0181 mol H in sample

Answer 1

Answer:

0.0136 mol  

Explanation:

C ⟶ CO₂

1. Moles of CO₂

$\text{Moles of CO}_{2} = \text{0.600 g CO}_{2} \times \dfrac{\text{1 mol CO}_{2}}{\text{44.01 g CO}_{2}} = \text{0.013 63 mol CO}_{2}$

2. Moles of C

$\text{Moles of C} = \text{0.013 63 mol CO}_{2} \times \dfrac{\text{1 mol C}}{\text{1 mol CO}_{2}} = \textbf{0.0136 mol C}$

Answer 2

Answer:

The amount of carbon is the sample is 0.163 grams.

Explanation:

Mass of carbon dioxide produced by the sample = 0.600 g

Moles of carbon dioxide = $\frac{0.600 g}{44 g/mol}=0.0136 mol$

Moles of carbon atom in 0.01364 moles of carbon dioxide:

1 × 0.0136 mol = 0.0136 mol

Mass of 0.01364 moles of carbon :

$=0.0136 mol\times 12 g/mol=0.163 g$

The amount of carbon is the sample is 0.163 grams.