Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction:
2CO + O2 yields 2CO2
Delta H for this reaction is -135.28 kcal.
If 811.7 kcal is released, how many moles of CO must have reacted?
1). 270.5 mol
2). 40.5 mol
3). 12.0 mol
4). 5.41 mol
5). 16.3 mol
6). 1.35 mol
7). 6.00 mol
135.37 kcal x # mol rxn = 811.7 kcal
# mol rxn = 6 but there are two mols CO in the rxn so 6*2 = 12 mol CO consumed.
To find out how many moles of CO must have reacted, we can use the heat released in the reaction and the enthalpy change of the reaction.
The enthalpy change (Delta H) for the reaction is given as -135.28 kcal. This means that for every 2 moles of CO that react, -135.28 kcal of heat is released.
We are given that 811.7 kcal is released. To find the number of moles of CO, we can set up a proportion using the enthalpy change:
-135.28 kcal / 2 moles CO = 811.7 kcal / x moles CO
Using cross multiplication, we can solve for x:
-135.28 kcal * x moles CO = 2 moles CO * 811.7 kcal
-135.28 x = 1623.4
x = -1623.4 / 135.28
x ≈ 12.0 mol
Therefore, the correct answer is option 3) 12.0 mol.
To determine the number of moles of CO that must have reacted, we can use the fact that the reaction releases 811.7 kcal, which is equal to -811.7 kcal (since it is released). We can set up a proportion using the known value for ΔH (-135.28 kcal) and the unknown number of moles of CO (x):
-811.7 kcal / -135.28 kcal = x mol / 2 mol
Simplifying the proportion:
6 = x / 2
Cross-multiplying:
6 * 2 = x
x = 12 mol
Therefore, the number of moles of CO that must have reacted is 12 mol. Thus, the correct answer is option 3), 12.0 mol.