[HRichyy]

EDIT:: Question is solved. I should not have been using q=mc deltaT. Not sure why I decided too, hahaha. The answer for those who care was pretty simple. Divide 112.40592 by 1000. Then divide 1.45 by .1124. That gives you the temperature change. I feel really stupid now for doing all that unnecessary work.




So I've been at this question for about 10-15 minutes now. Here's the question...

If 1.00 mole of ethanol, CH3CH2OH, at 22.0 °C absorbs 1.45 kJ of heat, what is the final temperature of the
ethanol? The specific heat capacity of ethanol is 2.44 J/g·K.

a. 9.1 °C                 d. 47.0 °C
b. 34.9 °C               e. 22.0 °C
c. 616 °C

I have done this problem many different ways and I keep getting 22.0°C
According to our answer sheet, this is wrong, it's 34.9°C

Here were some of the equations I tried.

45.06(2.44)(t-22) = 1.45

45.06(2.44)(t-22) = .99      (Got .99 from subtracting 1.45 from 2.44)

45.06(1.45)(t-22) = 2.44

45.06(1.45)(t-22) = .99

Every single equation leaves me with 22°C. Am I setting up the equation wrong? Not converting something correctly? Or is the answer right, and it's a typo on the answer sheet?

[sjb]

EDIT:: Question is solved. I should not have been using q=mc deltaT. Not sure why I decided too, hahaha. The answer for those who care was pretty simple. Divide 112.40592 by 1000. Then divide 1.45 by .1124. That gives you the temperature change. I feel really stupid now for doing all that unnecessary work.




So I've been at this question for about 10-15 minutes now. Here's the question...

If 1.00 mole of ethanol, CH3CH2OH, at 22.0 °C absorbs 1.45 kJ of heat, what is the final temperature of the
ethanol? The specific heat capacity of ethanol is 2.44 J/g·K.

a. 9.1 °C                 d. 47.0 °C
b. 34.9 °C               e. 22.0 °C
c. 616 °C

I have done this problem many different ways and I keep getting 22.0°C
According to our answer sheet, this is wrong, it's 34.9°C

Here were some of the equations I tried.

45.06(2.44)(t-22) = 1.45

45.06(2.44)(t-22) = .99      (Got .99 from subtracting 1.45 from 2.44)

45.06(1.45)(t-22) = 2.44

45.06(1.45)(t-22) = .99

Every single equation leaves me with 22°C. Am I setting up the equation wrong? Not converting something correctly? Or is the answer right, and it's a typo on the answer sheet?

For the benefit of others, where have the figures in your answer come from? I don't see 112.40592, 1000 or 1.45 anywhere in this question.

[Borek]

I should not have been using q=mc deltaT.

You definitely should use it to find the ΔT. Converting kJ to J would probably help you getting the right answer.

You are juggling numbers in hope some of the results will fit answer given. That almost never works - you don't understand WHY you got the right answer and you will be utterly lost when you will be given a problem without an answer.