Question

7.96 g of mgso₄ is placed into 100.0 ml of water. the water's temperature increases by 6.70 °c. calculate ∆h, in kj/mol, for the dissolution of mgso₄. (the specific heat of water is 4.184 j/g･ °c and the density of the water is 1.00 g/ml). you can assume that the specific heat of the solution is the same as that of water.

Answer 1

To calculate the ∆H, or heat of dissolution, for the dissolution of MgSO₄, we can use the formula q = mCΔT, where q is the heat transferred, m is the mass of the solution, C is the specific heat capacity of water, and ΔT is the change in temperature. The mass of the solution can be calculated by multiplying the density of water (1.00 g/ml) by the volume (100.0 ml) to get 100.0 g. The temperature change is given as 6.70 °C. Substituting these values into the formula, we get q = (100.0 g)(4.184 J/g °C)(6.70 °C) = 2799.28 J. To convert to kilojoules, we divide by 1000, so ∆H = 2.79928 kJ.

Step-by-step explanation:

To calculate the ∆H, or heat of dissolution, for the dissolution of MgSO₄, we can use the formula q = mCΔT, where q is the heat transferred, m is the mass of the solution, C is the specific heat capacity of water, and ΔT is the change in temperature. The mass of the solution can be calculated by multiplying the density of water (1.00 g/ml) by the volume (100.0 ml) to get 100.0 g. The temperature change is given as 6.70 °C.

Substituting these values into the formula, we get q = (100.0 g)(4.184 J/g °C)(6.70 °C) = 2799.28 J. To convert to kilojoules, we divide by 1000, so ∆H = 2.79928 kJ.