C6H12 = 9O2 --> 6CO2 = 6H2O + 3,690 kJ
*Personally Balanced*
What quantity of heat is produced if 32g of cyclohexane react with 95 L of oxygen at STP?
*My work so far is below*
95L*(1 mol O2/22.4L) = 4.2 mol O2
What would be the next motive?
I don't know what you next motive is but I suggest this for your next move. And note that I've corrected your equation for the typos.
C6H12 + 9O2 ==> 6CO2 + 6H2O
First determine what the limiting regent is.
mols cyclohexane = 32/84.2 = about 0.38
mols.
mols O2 from your work = 4.24
If 0.38 g cyclohexane reacts with an excess of O2, it will produce 0.38 x (6 mol CO2/1 mol C6H12) = about 2.28mol CO2.
If 4.24 mol O2 react with excess C6H12, CO2 produced is 4.24 x (6 mols CO2/9 mols O2) = 4.24 x 6/9 = about 2.83 mol CO2. Therefore, C6H12 is the limiting reagent and you have used all of it or 0.38 mols.
Then 1 mol produces 3690 kJ so you have
3690 kJ/mol x 0.38 mol = ? heat in kJ.
The next step would be to calculate the number of moles of cyclohexane using its molar mass. The molar mass of cyclohexane (C6H12) is 84.18 g/mol.
32 g of cyclohexane * (1 mol C6H12/84.18 g C6H12) = 0.38 mol C6H12
Now, we can use the balanced equation to find the amount of heat produced when 0.38 moles of cyclohexane react.
From the balanced equation, we know that 1 mole of cyclohexane produces 3,690 kJ of heat.
0.38 mol C6H12 * (3,690 kJ/1 mol C6H12) = 1,401.42 kJ
Therefore, 1,401.42 kJ of heat is produced when 32 g of cyclohexane reacts with 95 L of oxygen at STP.
The next step would be to determine the limiting reactant in the given reaction. To do this, you need to compare the number of moles of cyclohexane (C6H12) to the number of moles of oxygen (O2) that you calculated.
First, we need to find the number of moles of cyclohexane:
32g of cyclohexane * (1 mol C6H12/84.16g) = 0.381 mol C6H12
Now, compare the number of moles of cyclohexane (0.381 mol) to the number of moles of oxygen (4.2 mol). Since the stoichiometric ratio between cyclohexane and oxygen is 1:9, we can see that there are fewer moles of cyclohexane compared to oxygen.
Therefore, cyclohexane is the limiting reactant, which means that it will be completely consumed in the reaction, and there will be excess oxygen remaining.
Next, we can use stoichiometry to determine the amount of heat produced. From the balanced equation, we know that for every 1 mole of cyclohexane reacting, 3,690 kJ of heat is produced. Therefore, for 0.381 mol of cyclohexane, the amount of heat produced would be:
0.381 mol C6H12 * (3,690 kJ/1 mol C6H12) = 1,408.49 kJ
So, if 32g of cyclohexane react with 95 L of oxygen at STP, the quantity of heat produced would be approximately 1,408.49 kJ.