Question

14) 8 Carbon monoxide burns in oxygen to produce carbon dioxide.

2CO(g) + O2(g) → 2CO2(g)

Which mass of carbon dioxide is produced from 14 g of carbon monoxide?

A- 22 g

B- 28 g

C- 44 g

D- 88 g

Answer 1

A) 22

Step-by-step explanation:

The balanced chemical equation for the combustion of carbon monoxide tells us that:

2CO(g) + O2(g) → 2CO2(g)

This means that for every 2 moles of carbon monoxide (CO) that react, it produces 2 moles of carbon dioxide (CO2). Therefore, the molar ratio of CO to CO2 is 2:2, or simply 1:1.

To find the mass of CO2 produced from 14 g of CO, we first need to determine the number of moles of CO that are present in 14 g. The molar mass of CO is 28 g/mol (12 g/mol for carbon + 16 g/mol for oxygen).

Number of moles of CO = mass of CO / molar mass of CO

Number of moles of CO = 14 g / 28 g/mol

Number of moles of CO = 0.5 mol

Since the molar ratio of CO to CO2 is 1:1, we can conclude that 0.5 mol of CO will produce 0.5 mol of CO2.

Now, we can calculate the mass of CO2 produced from 0.5 mol of CO2:

Mass of CO2 = number of moles of CO2 x molar mass of CO2

Mass of CO2 = 0.5 mol x 44 g/mol (molar mass of CO2)

Mass of CO2 =22 g

Therefore, the correct answer is A) 22 g of carbon dioxide is produced from 14 g of carbon monoxide.

Hope this helps!