A15.0 g metal sample at 25.0 °c has 250 j of heat added to it. the specific heat of the metal is 0.128 j/g.°c. what is the final temperature?

The final temperature is

Explanation:

To calculate the final temperature, we use the equation:

where,

Q = heat absorbed = 250 J

m = Mass of the substance = 15 g

c = specific heat capacity of water = 0.128 J/g.°C

= change in temperature =

Putting values in above equation, we get:

Hence, the final temperature is

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"