contestada

Assume that 5.60 L of hydrogen gas at STP reacts with copper (II) oxide
according to the following balanced equation. How many grams of copper are produced?

CuO (s) + H2 (g) --> Cu (s) + H2O (g)

Respuesta :

Answer:

15.9 grams of copper is produced

Explanation:

Step 1: Data given

Volume of hydrogen = 5.60 L ( at STP)

Step 2: The balanced equation

CuO (s) + H2 (g) → Cu (s) + H2O (g)

Step 3: Calculate moles H2

22.4 L = 1 mol

5.60 L =  0.25 moles

Step 3: Calculate moles Cu

For 1 mol CuO we need 1 mol H2 to produce 1 mol Cu and 1 mol H2O

For 0.25 moles H2 we'll have 0.25 moles Cu

Step 4: Calculate mass Cu

Mass Cu = moles Cu * molar mass Cu

Mass Cu = 0.25 moles * 63.546 g/mol

Mass Cu = 15.9 grams

15.9 grams of copper is produced

Eduard22sly

The mass of copper, Cu produced from the reaction is 15.86 g

Determination of the mole of H₂

We'll begin by calculating the number of mole of H₂ that occupies 5.60 L at STP.

At standard temperature and pressure (STP),

22.4 L = 1 mole of H₂

Therefore,

5.60 L = 5.60 / 22.4

5.60 L = 0.25 mole of H₂

Determination of the mole of Cu from the reaction

CuO(s) + H₂(g) —> Cu(s) + H₂O(g)

From the balanced equation above,

1 mole of H₂ reacted to produce 1 mole of Cu.

Therefore,

0.25 mole of H₂ will also react to produce 0.25 mole of Cu.

How to determine the mass of Cu obtained from the reaction.

  • Molar mass of Cu = 63.5 g/mol
  • Mole of Cu = 0.25
  • Mass of Cu =?

Mass = mole × molar mass

Mass of Cu = 0.25 × 63.5

Mass of Cu = 15.86 g

Learn more about stoichiometry:

https://brainly.com/question/26311875