what are the steps to find the heat released in this problem?
and is the formula q=mc(deltaT)
36.0g of steam at 100.0degrees celcius(sp?) was condensed to water and cooled to 25.0degrees celcius(sp?). Find the heat released.
2007-10-28 06:05:18 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
First, condense the steam:
36.0gH2O x 539.6cal/g = 19425.6 cal = 19400 cal to three sig figs
Next cool the water through the 75degC temperature difference:
36.0gH2O x 75degC x 1cal/g-degC =2700 cal
Finally addemup:
19400cal + 2700cal = 22100cal total
2007-10-28 06:12:28 · answer #1 · answered by steve_geo1 7 · 0⤊ 0⤋
Hey there, can I get some help with this? Not sure what formula to use, and how to convert MJ per mole to KJ/g?
If the Heat of Combustion of Benzene (C6H6) is 4.25MJ per mole; How
much heat can I expect to be released if I burn 100g of Benzene knowing that
the Combustion Efficiency is only 80%. Show your workings.
2017-03-31 00:31:10 · answer #2 · answered by Felix 1 · 0⤊ 0⤋