A 1.0-g sample of MgCl2 produced a 10.00C increase in a calorimeter charged with 40.0mL of deionized water. The specific heat is of MgCl2 is 0.750J/C*g. What is the value of delta(s)H for MgCl2?
I know that the formula needed is delta(s)H=-([massH2O*deltaTH20]+[mass(MgCl2)*C(MgCl2)*deltaT(MgCl2)])/ Moles of MgCl2
How do you find the deltaT for the water and MgCl2? What is the C representing? Thanks in advance!
To find the deltaT for the water and MgCl2, you need to use the formula:
deltaT = final temperature - initial temperature.
In this case, the initial temperature is the same for both water and MgCl2, so you only need to find the final temperature. The given information is that the sample of MgCl2 caused a 10.00C increase in the calorimeter, which means the final temperature of the water is 10.00C higher than the initial temperature.
As for C, it represents the specific heat capacity. In this case, C(MgCl2) is the specific heat capacity of MgCl2, which is given as 0.750 J/C*g. This value tells you how much heat is needed to raise the temperature of 1 gram of MgCl2 by 1 degree Celsius.
To find the deltaT for water and MgCl2, you need to subtract the initial temperature from the final temperature. However, the problem statement does not provide the initial and final temperatures. Without this information, it is not possible to calculate deltaT.
C represents the specific heat capacity. In this problem, C(MgCl2) refers to the specific heat capacity of MgCl2, which is given as 0.750 J/C*g.