Question
How much energy is released when 73.0 g of ethylene reacts? Be sure your answer has the correct number of significant figures.
kcal released
kcal released
Answers
GPT 3.5
The molar mass of ethylene (C2H4) is 28.05 g/mol.
First, let's calculate the moles of ethylene in 73.0 g:
73.0 g / 28.05 g/mol = 2.60 mol
The balanced chemical equation for the combustion of ethylene is:
C2H4 + 3 O2 -> 2 CO2 + 2 H2O
From this equation, we see that 1 mole of C2H4 releases 141.8 kcal of energy.
So, for 2.60 moles of C2H4, the energy released would be:
2.60 mol * 141.8 kcal/mol = 369.08 kcal
Therefore, when 73.0 g of ethylene reacts, 369.08 kcal of energy is released. This value should be rounded to three significant figures, so the final answer is 369 kcal.
First, let's calculate the moles of ethylene in 73.0 g:
73.0 g / 28.05 g/mol = 2.60 mol
The balanced chemical equation for the combustion of ethylene is:
C2H4 + 3 O2 -> 2 CO2 + 2 H2O
From this equation, we see that 1 mole of C2H4 releases 141.8 kcal of energy.
So, for 2.60 moles of C2H4, the energy released would be:
2.60 mol * 141.8 kcal/mol = 369.08 kcal
Therefore, when 73.0 g of ethylene reacts, 369.08 kcal of energy is released. This value should be rounded to three significant figures, so the final answer is 369 kcal.