Question

Butane (C4H10) is burned in the presence of oxygen to form carbon dioxide and water.

Part: 0 / 2

Part 1 of 2

Write the balanced equation for the combustion of butane. Remember to include states of matter.

C4H10(g) + 02(g) -+ CO2(g) + H20(g)

How many liters of carbon dioxide are formed from 2.5 kg of butane at STP? Be sure your answer has the correct number of significant figures.
Note: Reference the SI prefixes table for additional information.

Answer 1

[AI-generated answer — Bot GPT 3.5]

To solve this problem, we first need to calculate the moles of butane (C4H10) based on the given mass of 2.5 kg.

1 mole of butane (C4H10) = 58.12 g
2.5 kg = 2.5 kg x 1000 g/kg = 2500 g

Now, calculate the moles of butane:
2500 g / 58.12 g/mol = 43.04 moles

According to the balanced equation, 1 mole of butane produces 4 moles of carbon dioxide. Therefore, the number of moles of carbon dioxide produced will be:
43.04 moles x 4 = 172.16 moles

Now we can use the ideal gas law to convert moles of carbon dioxide to liters at STP (Standard Temperature and Pressure):
1 mole of gas at STP occupies 22.4 L

172.16 moles x 22.4 L/mol = 3855.74 L

Therefore, 2.5 kg of butane will produce 3855.74 liters of carbon dioxide at STP.