Question

Use the following balanced reaction to answer the question:

P4 + 6Cl2 → 4PCl3

How many grams of phosphorus trichloride, PCl3, can be formed from the reaction of 30.0 grams of chlorine,Cl2?



58.1 g
38.7 g
87.2 g
77.5 g

Answer 1

38.7 g

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Answer 2

Answer: The mass of phosphorus trichloride produced is 58.1 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 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}=(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 =
`(4)/(6)* 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* 137.33g/mol)=58.1g`

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