Question

what volume of H2 at STP is required to reduce 0.795g of CuO to give Cu and H2O ?​

Answer 1

The volume of hydrogen gas required is 0.224 L

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of CuO = 0.795 g

Molar mass of CuO = 79.5 g/mol

Putting values in above equation, we get:

$\text{Moles of CuO}=\frac{0.795g}{79.5g/mol}=0.01mol$

The chemical equation for the reaction of CuO and hydrogen gas follows:

$CuO+H_2\rightarrow Cu+H_2O$

By Stoichiometry of the reaction:

1 mole of CuO reacts with 1 mole of hydrogen gas

So, 0.01 moles of CuO will react with = $\frac{1}{1}\times 0.01=0.01mol$ of hydrogen gas

At STP:

1 mole of a gas will occupy 22.4 L of volume

So, 0.01 moles of hydrogen gas will occupy = $\frac{22.4}{1}\times 0.01=0.224L$ of volume

Learn more about STP and number of moles:

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Answer 2

The volume of hydrogen gas required is 0.224 L

Explanation:

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}Number of moles=

Molar mass

Given mass

Given mass of CuO = 0.795 g

Molar mass of CuO = 79.5 g/mol

Putting values in above equation, we get:

\text{Moles of CuO}=\frac{0.795g}{79.5g/mol}=0.01molMoles of CuO=

79.5g/mol

0.795g

=0.01mol

The chemical equation for the reaction of CuO and hydrogen gas follows:

CuO+H_2\rightarrow Cu+H_2OCuO+H

2

→Cu+H

2

O

By Stoichiometry of the reaction:

1 mole of CuO reacts with 1 mole of hydrogen gas

So, 0.01 moles of CuO will react with = \frac{1}{1}\times 0.01=0.01mol

1

1

×0.01=0.01mol of hydrogen gas

At STP:

1 mole of a gas will occupy 22.4 L of volume

So, 0.01 moles of hydrogen gas will occupy = \frac{22.4}{1}\times 0.01=0.224L

1

22.4

×0.01=0.224L of volume