intro to chem

Calculate the amount of heat required to heat a 3.0kg gold bar from 23 degrees Celsius to 60 degrees Celsius

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asked by Carol
  1. q needed = mass Au x specific heat Au x (Tfinal-Tinitial)

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  2. Need to use 2 sig fig. Git 3.6x10 to the 1power. Computer says wrong. Any clues?

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    posted by Carol
  3. What did you use for specific heat Au? with units?

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  4. 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.

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  5. 0.128J

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    posted by Carol
  6. 0.128J/g C

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    posted by Carol
  7. Requests answer in 2 sig fig not 3

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    posted by Carol
  8. Would that make it 3.6x10 to the 3?

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    posted by Carol
  9. I don't understand how you get 3.6 anything.
    3000 x 0.128 x 37 = ?

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  10. .128x3000= 3.84x10E3 ?

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    posted by Carol
  11. Used 3.0x.128x37 which is difference os 23 to 60 degree change to get the 3.6

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    posted by Carol
  12. Need to drop kud at bday party will log in later

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    posted by Carol
  13. 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.

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  14. Thanks DeBob222

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    posted by Carol

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