Given the equation C2H4(g)+3O2(g)>2CO2(g)+2H2O(l)+1411kJ, how much heat is released when 8.00g of O2 react?
117.58kJ
To determine the amount of heat released when 8.00g of O2 reacts, we need to use the stoichiometry of the balanced chemical equation and the given enthalpy change of the reaction.
Step 1: Convert the given mass of O2 to moles.
The molar mass of O2 is 32.00 g/mol. Therefore, 8.00g of O2 is equal to 8.00g / 32.00 g/mol = 0.25 mol.
Step 2: Use the stoichiometry of the balanced equation to relate the moles of O2 to the moles of CO2 and the amount of heat released.
According to the balanced equation, 3 moles of O2 react to produce 2 moles of CO2 and release 1411 kJ of heat.
Therefore, to calculate the amount of heat released when 0.25 mol of O2 reacts, we can set up the following proportion:
(0.25 mol O2 / 3 mol O2) = (x kJ / 1411 kJ)
Solving for x, we get:
x = (0.25 mol O2 / 3 mol O2) * 1411 kJ = 117.58 kJ
So, when 8.00g of O2 react, approximately 117.58 kJ of heat is released.