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 = ?
.128x3000= 3.84x10E3 ?
Used 3.0x.128x37 which is difference os 23 to 60 degree change to get the 3.6
Need to drop kud at bday party will log in later
q = mass Au x specific heat Au x (Tfinal-Tinitial)
q = 3000 g x 0.128 J/g*c x 37C = 1.4 E4 J to two s.f.
If you multiply 3 x 0.128 x 37 you don't get 3.6. You get 14.2 BUT that 3 is not right. It is in kg and your specific heat unit is in J/g*c so you must change the 3 kg to 3000 g and use that.