How many dm³ of hydrogen, measured at s. t.p.,would be needed to reduce 47.7g of copper(II) oxide to copper? A. 4.48
B. 6.72
C. 10.82
D. 13.44

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D. 13.44 dm³

Explanation:

Step 1: Write the balanced equation

CuO + H₂ ⇒ Cu + H₂O

Step 2: Calculate the mass corresponding to 47.7 g of CuO

The molar mass of CuO is 79.55 g/mol.

47.7 g × (1 mol/79.55 g) = 0.600 mol

Step 3: Calculate the moles of H₂ that react with 0.600 mol of CuO

The molar ratio of CuO to H₂ is 1:1. The moles of H₂ are 1/1 × 0.600 mol = 0.600 mol.

Step 4: Calculate the volume of 0.600 moles of H₂ at STP

1 mol of any gas at STP has a volume of 22.4 dm³.

0.600 mol × (22.4 dm³/1 mol) = 13.44 dm³

it takes on an electronical energy