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

The amount of carbon is the sample is 0.163 grams.

Step-by-step explanation:

Mass of carbon dioxide produced by the sample = 0.600 g

Moles of carbon dioxide =
`(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* 12 g/mol=0.163 g`

The amount of carbon is the sample is 0.163 grams.

Answer 2

0.0136 mol

Step-by-step explanation:

C ⟶ CO₂

1. Moles of CO₂

`\text{Moles of CO}_(2) = \text{0.600 g CO}_(2) * \frac{\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) * \frac{\text{1 mol C}}{\text{1 mol CO}_(2)} = \textbf{0.0136 mol C}`