Question

Be sure to answer all parts. Barium carbonate decomposes upon heating to barium oxide and carbon dioxide. Enter and balance the equation (including the physical states) Calculate the number of g of carbon dioxide produced by heating 71.0 g of barium carbonate. g CO2

Answer 1

Answer: The mass of carbon dioxide produced is 15.8 grams

Step-by-step explanation:

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

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}` ......(1)

Mass of barium carbonate = 71.0 grams

Molar mass of barium carbonate = 197.34 g/mol

Putting values in equation 1:, we get:

`\text{Moles of }BaCO_3=(71.0g)/(197.34g/mol)=0.360mol`

The chemical equation for the decomposition of barium carbonate follows:

`BaCO_3(s)\rightarrow BaO(s)+CO_2(g)`

By Stoichiometry of the reaction:

1 mole of barium carbonate produces 1 mole of carbon dioxide.

So, 0.360 moles of barium carbonate will produce =
`(1)/(1)* 0.360=0.360mol` of carbon dioxide.

Now, calculating the mass of carbon dioxide by using equation 1, we get:

Moles of carbon dioxide = 0.360 mol

Molar mass of carbon dioxide = 44 g/mol

Putting values in equation 1, we get:

`0.360mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(0.360mol* 44g/mol)=15.8g`

Hence, the mass of carbon dioxide produced is 15.8 grams