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3 years ago

Can 1750 mL of water dissolve 4.6 moles of copper sulfate CuSO4

Chemistry

1 answer:

amm18123 years ago

8 0

Answer:

Explanation:

We first find the solubility of the copper sulphate salt

Number of moles= 4.6 moles

Volume =1.75 L

Molarity= number of moles/ volume = 4.6/1.75= 2.6 molL-1

Hence, only 2.6 moles of Copper II sulphate dissolves in 1.75L of water. Hence 4.6 moles of copper II Sulphate dies not dissolve in 1.75 L of water.

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Answer:

The volume of the vessel is 250 L

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Explanation:

Using Boyle's law

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Using above equation as:

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${V_2}=\frac {{25}\times {20.0}}{2}\ L$

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<u>The volume of the vessel is 250 L.</u>

According to Dalton's law of partial pressure:-

$P_{H_2}=Mole\ fraction\times Total\ Pressure$

So, according to definition of mole fraction:

$Mole\ fraction\ of\ H_2=\frac {n_{H_2}}{n_{H_2}+n_{He}}$

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3 years ago