Asked by Anonymous
In a calorimeter experiment done at constant pressure in which all the heat from a chemical reaction was absorbed by the surrounding water bath, the temperature of the water went up by 2.31 K. If the size of the water bath was 200 g, what was the amount of heat transferred to the water? If the chemical reaction was
CH4(g) + 2O2(g) --> CO2(g) + 2H2O(l)
and 2.17x1-^-3 moles of CH4 were burned, what is DH for the reaction?
I got 1.00J
CH4(g) + 2O2(g) --> CO2(g) + 2H2O(l)
and 2.17x1-^-3 moles of CH4 were burned, what is DH for the reaction?
I got 1.00J
Answers
Answered by
DrBob222
Off hand I wouldn't think so.
q = mass H2O x specific heat H2O x delta T = ?,I think the question is stated improperly. This is the dH for the reaction as shown. What the problem wants, I think, is dH for the reaction/mol. That is
Then q/mol CH4 = dH for the reaction. I get something like 890 kJ/mol.
q = mass H2O x specific heat H2O x delta T = ?,I think the question is stated improperly. This is the dH for the reaction as shown. What the problem wants, I think, is dH for the reaction/mol. That is
Then q/mol CH4 = dH for the reaction. I get something like 890 kJ/mol.
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