Question

A compound contains only carbon, hydrogen, and oxygen. Combustion of 65.76 g of the compound yields 96.38 g of CO2 and 39.46 g of H2O.
The molar mass of the compound is 90.078 g/mol.
1. Calculate the grams of carbon (C) in 65.76 g of the compound:
2. Calculate the grams of hydrogen (H) in 65.76 g of the compound.
3. Calculate the grams of oxygen (O) in 65.76 g of the compound.

Answer 1

Answer:

1. 26.30 g C.

2. 4.42 g H.

3. 35.04 g O.

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to calculate the required as follows:

1. Here, the only source of carbon is in CO2, and thus, we calculate the grams of carbon from the produced grams of this substance:

$m_C=96.38gCO_2*\frac{1molCO_2}{44.01gCO_2} *\frac{1molC}{1molO_2} *\frac{12.01gC}{1molC} =26.30g$

2. Here, the only source of hydrogen is in H2O, and thus, we calculate the grams of hydrogen from the produced grams of this substance:

$m_H=39.46gH_2O*\frac{1molH_2O}{18.02gH_2O} *\frac{2molH}{1molH_2O} *\frac{1.01gH}{1molH} =4.42gH$

3. Here, we subtract the mass of H and C from the mass of the sample, to obtain the mass of oxygen:

$m_O=65.76g-26.30g-4.42g\\\\m_O=35.04g$

Regards!