Question

Using the balanced equation for the combustion of acetylene, answer the following questions. 2 H―C≡C―H + 5 O2 → 4 CO2 + 2 H2O acetylene How many grams of CO2 are formed from 2.2 mol of C2H2? How many grams of CO2 are formed from 0.69 mol of C2H2?

Answer 1

To determine the grams of CO2 formed from a given number of moles of C2H2 (acetylene), we need to use the balanced equation and the molar ratios between C2H2 and CO2.

The balanced equation for the combustion of acetylene is: 2 H―C≡C―H + 5 O2 → 4 CO2 + 2 H2O

According to the balanced equation, for every 2 moles of C2H2, 4 moles of CO2 are produced. This gives us the molar ratio of C2H2 to CO2 as 2:4, or simply 1:2.

Now, let's calculate the grams of CO2 formed for each given number of moles of C2H2:

1. For 2.2 mol of C2H2: Using the molar ratio of 1:2 (C2H2:CO2), we can calculate: 2.2 mol C2H2 * (4 mol CO2 / 2 mol C2H2) * (molar mass of CO2)

The molar mass of CO2 is approximately 44.01 grams/mol.

Calculating: 2.2 mol * (4 mol CO2 / 2 mol C2H2) * 44.01 g/mol = 176.04 grams of CO2

Therefore, 2.2 mol of C2H2 will produce approximately 176.04 grams of CO2.

2. For 0.69 mol of C2H2: Using the molar ratio of 1:2 (C2H2:CO2), we can calculate: 0.69 mol C2H2 * (4 mol CO2 / 2 mol C2H2) * (molar mass of CO2)

Calculating: 0.69 mol * (4 mol CO2 / 2 mol C2H2) * 44.01 g/mol = 60.46 grams of CO2

Therefore, 0.69 mol of C2H2 will produce approximately 60.46 grams of CO2.