Suppose you add 81 ml of dilute acid to 54 ml of water. Both the water and acid were at room temperature (22 C) before being mixed. The temperature of the solution increased to 42 C. How much energy (in kJ) was released by the dissolution of the acid if the specific heat capacity of the solution is still the same as water 4.18 J/(gK) and the density was still approximately 1.0 g/ml.

Heat= totalmass*c*changeinTemp

can you do it now?

To determine the amount of energy released by the dissolution of the acid, we need to calculate the change in temperature of the solution and the amount of solution for which the temperature increased.

First, let's calculate the change in temperature:

ΔT = Tfinal - Tinitial
= 42°C - 22°C
= 20°C

Next, let's determine the mass of the solution. Since the density of the solution is approximately 1.0 g/mL:

Mass = Volume × Density
= (81 mL + 54 mL) × 1.0 g/mL
= 135 g

Now, we can calculate the amount of energy released using the equation:

Energy released = mass × specific heat capacity × temperature change

Convert the mass to grams:

Mass = 135 g

Substitute the values into the equation:

Energy released = 135 g × 4.18 J/(g·K) × 20°C

Now, we need to convert the units to kJ:

1 kJ = 1000 J

Energy released = (135 g × 4.18 J/(g·K) × 20°C) / (1000 J/kJ)
= (135 × 4.18 × 20) / 1000 kJ
= 11.286 kJ

Therefore, approximately 11.286 kJ of energy was released by the dissolution of the acid.