4130 J of energy is added to a 52 g sample of water that has an initial temperature of 10.0°C. If the specific heat of water is 4.18 J/(g × °C), what would the final temperature of the water be?

10°C

19°C

29°C

51°C

Question

4130 J of energy is added to a 52 g sample of water that has an initial temperature of 10.0°C. If the specific heat of water is 4.18 J/(g × °C), what would the final temperature of the water be?

 10°C

 19°C

 29°C

 51°C

anonymous · Answer

somewhere i am calculating this wrong i keep getting 33.19

jfraser · Answer

I get a change in temperature of 19C, so if the temp started at 10C, and increased by 19C, the final temp is quite clear

jfraser · Answer

I used $$Q = m*C*\Delta T$$

anonymous · Answer

⌂

anonymous · Answer

hmmm. i didnt even know about the way you used.

jfraser · Answer

how did you try to solve it, if you didn't use that equation?