Respuesta :
Answer:
13.44 dm³ of hydrogen is needed for the reaction.
(D) is correct option
Explanation:
Given that,
Mass of copper(II) oxide = 47.7 g
We know that,
Molar mass of CuO = 63.5 + 16 = 79.5 g/mol
We need to calculate the number of moles in 47.7g of copper(II) oxide,
Using formula of moles
[tex]mole=\dfrac{mass}{molar\ mass}[/tex]
Put the value into the formula
[tex]moles=\dfrac{47.7}{79.5}[/tex]
[tex]moles=0.6\ mole[/tex]
Now, we write the balanced equation for the reaction
[tex]CuO+H_{2}\Rightarrow Cu+H_{2}O[/tex]
Here, one mole of CuO reacted with one mole of hydrogen to produce one mole of Cu and one mole of water.
We need to calculate the number of moles of hydrogen needed to react with 0.6 mole of copper(II) oxide
Using the balanced equation,
1 mole of CuO reacted with 1 mole of Hydrogen.
Therefore, 0.6 mole of CuO will also react with 0.6 mole of hydrogen.
We need to calculate the volume of occupied by 0.6 mole of H2 at STP
Using formula of volume
[tex]n=\dfrac{V}{V'}[/tex]
Where, n = mole of hydrogen
V = occupied volume
V'= volume at STP
Put the value into the formula
[tex]0.6=\dfrac{V}{22.4}[/tex]
[tex]V=0.6\times22.4[/tex]
[tex]V=13.44\ dm^3[/tex]
Hence, 13.44 dm³ of hydrogen is needed for the reaction.
