Copper is extracted from copper oxide by reacting coppor oxide with carbon. Figure 2 shows the apparatus. Figure 2 The equation for the reaction is: 2CuO(s)+C(s)arrow 2Cu(s)+CO_(2)(g) In an experiment 15.9 g of copper oxide and 1.2 g of carbon reacted. 12.7 g of copper was produced in the reaction. (f) Calculate the mass of carbon dioxide produced in this experiment. __

Question

Answer 1

# Explanation:## Step 1:Identify the given quantities and the chemical equation. The chemical equation for the reaction is:

Given:- Mass of copper oxide (

) =

- Mass of carbon (

) =

- Mass of copper (

) produced =

## Step 2:Calculate the molar masses of the reactants and products:- Molar mass of

= \(63.55 \, (\mathrm{Cu}) + 16.00 \, (\mathrm{O}) = 79.55 \, \mathrm{g/mol}\)- Molar mass of

=

- Molar mass of

=

- Molar mass of

= \(12.01 \, (\mathrm{C}) + 2 \times 16.00 \, (\mathrm{O}) = 44.01 \, \mathrm{g/mol}\)## Step 3:Determine the moles of

and

used in the reaction:

## Step 4:Identify the limiting reactant. According to the balanced equation, 2 moles of

react with 1 mole of

. Therefore:

Since the moles of

available (0.2 mol) match exactly with the requirement,

is the limiting reactant.## Step 5:Calculate the moles of

produced using the stoichiometry of the reaction. From the balanced equation, 2 moles of

produce 1 mole of

:

## Step 6:Calculate the mass of

produced:

# Answer:The mass of carbon dioxide produced in this experiment is

.

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