You mix 5.32 g of solid magnesium sulfate with 105.24 g of water inside a calorimeter. As the magnesium sulfate dissolves, the temperature of the solution rises from 24.5°C to 30.1°C. Calculate the amount of energy in kJ that was transferred into the surroundings through heating. Assume that the specific heat capacity of the solution is 4.18 J/g·°C.

kJ

q = mass H2O x specific heat H2O x (Tfinal-Tinitial)

Since this is an exothermic reaction, the prof MAY want a negative sign on it; one never knows. I wouldn't use one since if heat is being transferred into the surroundings it MUST have been exothermic.

Idk what the answer is does anyone know

To calculate the amount of energy transferred into the surroundings through heating, we need to use the formula:

q = m * c * ΔT

Where:
q = amount of energy transferred (in joules or J)
m = mass of the solution (in grams)
c = specific heat capacity of the solution (in J/g·°C)
ΔT = change in temperature (final temperature - initial temperature) (in °C)

First, we need to calculate the mass of the solution. This can be done by adding the mass of the solid magnesium sulfate (5.32 g) to the mass of the water (105.24 g). So:

Mass of solution = mass of solid + mass of water
= 5.32 g + 105.24 g
= 110.56 g

Now we can substitute the values into the formula:

q = (110.56 g) * (4.18 J/g·°C) * (30.1°C - 24.5°C)

Simplifying:

q = (110.56 g) * (4.18 J/g·°C) * (5.6°C)

Calculating:

q = 1310.44 J

To convert from joules to kilojoules, divide by 1000:

q = 1310.44 J / 1000
= 1.31 kJ

Therefore, the amount of energy transferred into the surroundings through heating is 1.31 kJ.