It appears that you need help with a chemistry question related to the gas-phase reaction of ethylene (C2H4) with hydrogen (H2) to form ethane (C2H6) in the presence of a palladium catalyst. Let’s tackle this together!
The given reaction is as follows:
C2H4+H2→C2H6
How much energy is released when 52.0 of ethylene reacts? Be sure your answer has the correct number of significant figures.
To determine the amount of energy released when 52.0 grams of ethylene reacts, we first need to calculate the moles of ethylene involved in the reaction.
1. Calculate the molar mass of ethylene (C2H4):
C: 12.01 g/mol
H: 1.008 g/mol
Molar mass of C2H4 = 2(12.01) + 4(1.008) = 28.054 g/mol
2. Calculate the number of moles in 52.0 grams of C2H4:
52.0 g / 28.054 g/mol ≈ 1.853 moles
3. The balanced chemical equation tells us that the reaction of 1 mole of ethylene releases a certain amount of energy. Therefore, we can use the given stoichiometry of the reaction to determine the amount of energy released for 1.853 moles of ethylene.
From the balanced equation: 1 mol C2H4 releases x amount of energy
From the reaction stoichiometry: 1 mol C2H4 = 1 mol C2H6 (ethane) released (energy change is the same)
Therefore, we can assume that each mole of C2H4 released 284 kJ of energy.
4. Calculate the energy released for 1.853 moles of ethylene:
1.853 moles x 284 kJ/mol = 526.852 kJ
Therefore, when 52.0 grams of ethylene react, approximately 526.852 kJ of energy is released. Keeping in mind the given number of significant figures (3 significant figures), the final answer should be 527 kJ.