Question

Refer to the following unbalanced equation: CO2 H20 C6H14 O2>CO2 + H2O What mass of oxygen (O2) is required to react completely with 10.4 g of C6H14? D. 36.7 g Selected Answer: D. 36.7 g Correct Answer:

Answer 1

Answer: The mass of oxygen gas required is 36.7 grams.

Step-by-step explanation:

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

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}` .....(1)

Given mass of hexane = 10.4 g

Molar mass of hexane = 86.18 g/mol

Putting values in equation 1, we get:

`\text{Moles of hexane}=(10.4g)/(86.18g/mol)=0.12mol`

The chemical equation for the combustion of hexane follows:

`2C_6H_(14)+19O_2\rightarrow 12CO_2+14H_2O`

By stoichiometry of the reaction:

2 moles of hexane reacts with 19 moles of oxygen gas

So, 0.12 moles of hexane will react with =
`(19)/(2)* 0.12=1.14mol` of oxygen gas.

Now, calculating the mass of oxygen gas by using equation 1, we get:

Molar mass of oxygen gas = 32 g/mol

Moles of oxygen gas = 1.14 moles

Putting values in equation 1, we get:

`1.14mol=\frac{\text{Mass of oxygen gas}}{32g/mol}\\\\\text{Mass of oxygen gas}=36.7g`

Hence, the mass of oxygen gas required is 36.7 grams.