Question

According to the following reaction, how many grams of oxygen gas are required for the complete reaction of 30.3 grams of hydrochloric acid? hydrochloric acid (aq) + oxygen (g) water (l) + chlorine (g) grams oxygen gas

Answer 1

Answer: The mass of oxygen gas required will be 6.648 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 hydrochloric acid = 30.3 g

Molar mass of hydrochloric acid = 36.46 g/mol

Putting values in above equation, we get:

`\text{Moles of }HCl=(30.3g)/(36.46g/mol)=0.831mol`

For the given chemical reaction, the balanced equation follows:

`4HCl+O_2\rightarrow 2H_2O+2Cl_2`

By Stoichiometry of the reaction:

4 moles of HCl reacts with 1 mole of oxygen gas.

So, 0.831 moles of HCl will react with =
`(1)/(4)* 8.31=0.20775mol` of oxygen gas.

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

Moles of oxygen gas = 0.20775 moles

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

`0.20775mol=\frac{\text{Mass of oxygen gas}}{32g/mol}\\\\\text{Mass of oxygen gas}=6.648g`

Hence, the mass of oxygen gas required will be 6.648 grams.