Asked by kika
A coffee cup calorimeter contains 100.0 g of
water at 10.0 ◦C. A 72.4 g sample of iron
is heated to 100 ◦C and dropped into the
calorimeter. Assuming there is no heat lost
to the coffee cup, calculate the final temperature
of the system. The specific heats of iron
and water are 0.449 J/g ◦C and 4.184 J/g ◦C,
respectively.
water at 10.0 ◦C. A 72.4 g sample of iron
is heated to 100 ◦C and dropped into the
calorimeter. Assuming there is no heat lost
to the coffee cup, calculate the final temperature
of the system. The specific heats of iron
and water are 0.449 J/g ◦C and 4.184 J/g ◦C,
respectively.
Answers
Answered by
DrBob222
heat lost by Fe + heat gained by H2O = 0
[mass Fe x specific heat Fe x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0
Substitute and solve for Tfinal.
[mass Fe x specific heat Fe x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0
Substitute and solve for Tfinal.
Answered by
Anonymous
45.3 C
Answered by
Anonymous
16.5 is the answer.
Whoever said 45.3 is an actual dunce
Whoever said 45.3 is an actual dunce
Answered by
Anonymous
Its 16.5 C
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