Question

For CH4+2O2→CO2+2H2O, the molar mass of oxygen gas (02) is 32.00 g/mol. The molar mass of carbon dioxide (CO2) is 44.01 g/mol. What mass of CO2, in grams, will form when 8.94 g O2 completely react?

Answer 1

The balanced chemical equation tells us unequivocally that 16 g of methane gas reacts with 32 g of dioxygen gas to give 44 g of carbon dioxide, and 36 g of water. These masses represent the molar equivalence of reactants and products. You have to work the molar quantity of the given mass of dioxygen, and with how much methane it will react.

Answer 2

Mass of $CO_2$ in grams that will form when 8.94 g oxygen completely react is 6.2 g.

Explanation:

To calculate the number of mole, we use the equation:

$\text{Number of mole}=\frac{\text{Given mass}}{\text{Molar mass}}$  

For oxygen:

Given mass of oxygen = 8.94 g

Molar mass of oxygen = 32 g/mol

Putting values we get:

Moles of oxygen=$\frac{8.94g}{32g/mol}=0.28mol$

The chemical equation for the reaction follows:

$CH_4+2O_2\rightarrow CO_2+2H_2O$

By Stoichiometry of the reaction:

2 moles of oxygen react to produce =  1 mole of carbon dioxide

So, 0.28 moles of oxygen react to produce = $\frac{1}{2}\times 0.28=0.14mol$ of carbon dioxide

$0.14mol=\frac{\text{Mass of carbon dioxide}}{44.01g/mol}\\\\\text{Mass of carbon dioxide}=6.2g$

Thus mass of $CO_2$  that will form is 6.2 g

Learn more about stoichiometry

https://brainly.in/question/11902840

https://brainly.com/question/13645176