What quantity of heat is required to produce 5 mol of oxygen gas by this reaction? HgO(s) → Hg(l) + ½ O2(g), ΔH = +90.7kJ
I calculated 90.7*5, but my online homework says its wrong how do I calcuate this?
907.5 kJ
What do you have to multiply ½ O2 by to get 5 moles of O2?
1/2x=5
Solving for x
x=10, so you have to multiply O2 and everything else by 10 to get the following:
10HgO(s) → 10Hg(l) +5O2(g), ΔH = +907kJ not 907.5 kj. I apologize, a typo in my original response.
907
To calculate the quantity of heat required to produce 5 mol of oxygen gas, you need to apply the concept of stoichiometry. The balanced equation you provided is:
HgO(s) → Hg(l) + ½ O2(g)
From the equation, you can see that for every 1 mol of HgO(s) that reacts, ½ mol of O2(g) is produced. Therefore, you can set up the following ratio:
1 mol HgO(s) : ½ mol O2(g) = 90.7 kJ
To find the quantity of heat required to produce 5 mol of O2(g), you need to multiply the given ratio by the appropriate factor. In this case, you want to find the heat for 5 mol of O2(g), so you need to multiply the ratio by 5:
1 mol HgO(s) : ½ mol O2(g) = 90.7 kJ
(5 mol O2(g)) / (½ mol O2(g)) = 10
Now, multiply the ratio by the factor of 10:
10 × 90.7 kJ/mol = 907 kJ
Therefore, the quantity of heat required to produce 5 mol of oxygen gas is 907 kJ, not 90.7 kJ.
I apologize for the confusion caused by the incorrect calculation.