The enthalpy change for the reaction of ethylene with hydrogen to form ethane is -136.2 kcal/mol.
First, we need to calculate the moles of ethylene in 21.0 g.
Molar mass of C2H4 = 2(12.01) + 4(1.008) = 28.05 g/mol
Moles = 21.0 g / 28.05 g/mol = 0.749 mol
Now, we can calculate the energy released when 0.749 mol of ethylene reacts.
Energy released = 0.749 mol x (-136.2 kcal/mol) = -101.9 kcal
Therefore, 101.9 kcal of energy is released when 21.0 g of ethylene reacts.
Consider the gas-phase reaction of ethylene (C2H4) with hydrogen (H2) to form ethane (C2H6), which occurs in the presence of a palladium catalyst.
Part: 0 / 7
Part 1 of 7
Write a balanced equation for this equilibrium. Do not include the palladium catalyst. Include all physical states of matter.
C2H4(g)+ H2(g)= C2H6 (g)
x
Part: 1 / 7
How much energy is released when 21.0 g of ethylene reacts? Be sure your answer has the correct number of significant figures.
kcal released
1 answer