Calculate the amount of heat required to heat a 3.0kg gold bar from 23 degrees Celsius to 60 degrees Celsius
q needed = mass Au x specific heat Au x (Tfinal-Tinitial)
Need to use 2 sig fig. Git 3.6x10 to the 1power. Computer says wrong. Any clues?
What did you use for specific heat Au? with units?
I'm guessing here since I don't know what you used for specific heat Au and what units you want the answer. But my guess is you used specific heat in cal/g*C and that's about 0.032. delta T is 60-23 = 37. Then I think you failed to convert 3 kg Au to g Au so
3 x 0.032 x 37 = about 36 which is your answer. You should use 3000. Also note that your answer of 3.6E1 is not three significant figures.
3000 x 0.032 x 37 = 3.55E3 calories or close to that depending upon your value for sp.h.
0.128J
0.128J/g C
Requests answer in 2 sig fig not 3
Would that make it 3.6x10 to the 3?
I don't understand how you get 3.6 anything.
3000 x 0.128 x 37 = ?