Question

How many liters of CO₂ are formed during the combustion of 120.0 grams of ethane at stp in the open atmosphere?

Answer 1

To find the number of liters of CO₂ formed during the combustion of ethane, we first need to convert the mass of ethane to moles. We do this by dividing the given mass by the molar mass of ethane. Then, we use the balanced chemical equation for the combustion of ethane to determine the mole ratio between ethane and CO₂. Finally, we convert moles of CO₂ to liters by multiplying the moles by the molar volume of a gas at STP. Therefore, approximately 89.47 liters of CO₂ are formed during the combustion of 120.0 grams of ethane at STP in the open atmosphere.

Step-by-step explanation:

To find the number of liters of CO₂ formed during the combustion of ethane, we first need to convert the mass of ethane to moles. We do this by dividing the given mass by the molar mass of ethane. Then, we use the balanced chemical equation for the combustion of ethane to determine the mole ratio between ethane and CO₂. Finally, we convert moles of CO₂ to liters by multiplying the moles by the molar volume of a gas at STP.

Let's go through the calculations:

1. Convert grams of ethane to moles: (120.0 g ethane) / (30.07 g/mol) = 3.989 moles ethane
2. Use the mole ratio from the balanced chemical equation: 2 moles ethane produce 4 moles CO₂
3. Convert moles of CO₂ to liters at STP: (3.989 moles CO₂) * (22.414 L/mol) = 89.47 L CO₂

Therefore, approximately 89.47 liters of CO₂ are formed during the combustion of 120.0 grams of ethane at STP in the open atmosphere.