Can someone help me how to go through this problem or how to start ?

Chemistry
Tutor: None Selected Time limit: 1 Day

A 150.0-g sample of a metal at 27.9°C is added to 150.0 g of H2O at 13.1°C. The temperature of the water rises to 15.7°C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water.

 J °C−1 g−1
Oct 10th, 2015

Where H is the specific heat capacity

Solve this equation for the specific heat capacity of the metal (H_metal), then plug in the values

Oct 10th, 2015

Ok so,   150 + x + (15.7-27.9) + ( 150 * ?* (15.7- 13.1) ) = 0
What would the H of H20 be ? 

Oct 10th, 2015

The specific heat of water is (4.18 J/g*degrees C)

Oct 10th, 2015

Ok thanks , oh and the beginning part of the formula is multiplication not addition 

Oct 10th, 2015

Ah yeah it is apologies

Oct 10th, 2015


Oct 10th, 2015
fix.png

Ok for the ice problem it's the same calculation, but I simplified this one, just make sure to carry the negative signs properly to get the right answer.

Oct 10th, 2015


Oct 10th, 2015
equation3.png

Thanks sooo much , I really appreciate it. 

Oct 11th, 2015

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Oct 10th, 2015
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