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 (change in temperature) for water and MgCl2, you need to subtract the initial temperature from the final temperature.
However, in the given problem statement, the initial and final temperatures for water and MgCl2 are not provided. To calculate the deltaT for water, you need to know the initial and final temperatures of water before and after the addition of MgCl2. Similarly, you need the initial and final temperatures of the calorimeter to calculate the deltaT for MgCl2.
The specific heat, denoted by "C," represents the amount of heat energy required to raise the temperature of a substance by one degree Celsius. In this problem, C(MgCl2) represents the specific heat of MgCl2, which is given as 0.750 J/C*g.
So, to find delta(s)H for MgCl2, you can use the formula:
delta(s)H = -([massH2O * deltaT(H2O)] + [mass(MgCl2) * C(MgCl2) * deltaT(MgCl2)]) / Moles of MgCl2
You need to substitute the corresponding values for massH2O, deltaT(H2O), mass(MgCl2), C(MgCl2), and Moles of MgCl2 to calculate delta(s)H for MgCl2.