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Question 1
Indicate the answer choice that best completes the statement or answers the question
How many grams of chlorine gas can be produced from the decomposition of 73.4 g. of AuCl2 by this reaction
2AuClz - 2 Au + 3 Cl2

Answer 1

Answer: 25.8 g of
`Cl_2` will be produced from the decomposition of 73.4 g of
`AuCl_3`

Step-by-step explanation:

To calculate the moles :

`\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}`

`\text{Moles of} AuCl_3=(73.4g)/(303g/mol)=0.242moles`

The balanced chemical reaction is:

`2AuCl_3\rightarrow 2Au+3Cl_2`

According to stoichiometry :

2 moles of
`AuCl_3` produce = 3 moles of
`Cl_2`

Thus 0.242 moles of will produce=
`(3)/(2)* 0.242=0.363mol` of
`Cl_2`

Mass of
`Cl_2`=
`moles* {\text {Molar mass}}=0.363mol* 71g/mol=25.8g`

Thus 25.8 g of
`Cl_2` will be produced from the decomposition of 73.4 g of
`AuCl_3`