Question

Use the following balanced reaction to answer the question:

Answer 1

Answer: The mass of phosphorus trichloride produced is 58.1 grams.

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 chlorine gas = 30.0 g

Molar mass of chlorine gas = 71 g/mol

Putting values in equation 1, we get:

$\text{Moles of chlorine gas}=\frac{30.0g}{71g/mol}=0.422mol$

The given chemical equation follows:

$P_4+6Cl_2\rightarrow 4PCl_3$

By Stoichiometry of the reaction:

6 moles of chlorine gas produces 4 moles of phosphorus trichloride

So, 0.422 moles of chlorine gas will produce = $\frac{4}{6}\times 0.422=0.281mol$ of phosphorus trichloride

Now, calculating the mass of phosphorus trichloride from equation 1, we get:

Molar mass of phosphorus trichloride = 137.33 g/mol

Moles of phosphorus trichloride = 0.422 moles

Putting values in equation 1, we get:

$0.422mol=\frac{\text{Mass of phosphorus trichloride}}{137.33g/mol}\\\\\text{Mass of phosphorus trichloride}=(0.422mol\times 137.33g/mol)=58.1g$

Hence, the mass of phosphorus trichloride produced is 58.1 grams.

Answer 2

Answer:

38.7 g

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