Question

Balance the equation and show the calculation of the number of moles and grams of CO2 formed from 11.9 grams of O2. Show your answers to 3 significant figures. C6H14 + O2 → CO2 + H2O

Answer 1

Answer:

0.2349 moles, 10.3356 g

Explanation:

The given reaction is :

$C_6H_{14}+O_2\rightarrow CO_2 + H_2O$

The balanced reaction by equating the same number of each atom both side is :

$2C_6H_{14}+19O_2\rightarrow 12CO_2 + 14H_2O$

Given that :

Amount of oxygen gas = 11.9 g

Molar mass of oxygen gas = 32 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus, moles are:

$moles= \frac{11.9\ g}{32\ g/mol}$

$moles= 0.3719\ mol$

From the reaction,  

19 moles of oxygen gas on reaction forms 12 moles of carbon dioxide

Also,

1 mole of oxygen gas on reaction forms 12/19 moles of carbon dioxide

So,

0.3719 moles of zinc on reaction forms $\frac {12}{19}\times 0.3719$ mole of carbon dioxide

Moles of carbon dioxide formed = 0.2349 moles

Mass of carbon dioxide = moles×Molar mass

Molar mass of carbon dioxide = 44 g/mol

Mass of carbon dioxide formed = 0.2349 ×44 g = 10.3356 g