When 10.00 ml of 1.00 m hcl solution is mixed with 115 ml of 0.100 m naoh solution in a constant-pressure calorimeter, the temperature rises from 22.45 °c to 23.25 °
c. calculate q for this reaction, assuming that the heat capacity of the calorimeter is the same as that of 125 g of water.?

The amount of energy required by the reaction is .

Further Explanation:

Given:

The volume of  mixed in the calorimeter is .

The volume of  mixed in the calorimeter is .

The initial temperature of the solution is  or .

The final temperature of the solution is  or .

The specific heat capacity of water is .

Concept:

The total volume of the calorimeter after the addition of   and  is:

The density of the given solution is . Therefore, the mass of the solution is:

The change in temperature of the calorimeter is.

Now, the amount of heat absorbed by the calorimeter to complete the reaction is given as:

Here,   is the amount of heat required for the reaction and  is the heat capacity of the calorimeter.

Substitute the values in the above expression.

Thus, the amount of energy required by the reaction is .

Learn More:

1. One consequence of the third law of thermodynamics is that

2. According to Charles’s law, for a fixed quantity of gas at constant pressure

3. Calculate the average translational kinetic energy (sometimes just called average kinetic energy)

Answer Details:

Grade: High School

Subject: Physics

Chapter: Heat and Thermodynamics

Keywords:

10 ml of 1.00 m HCl, 115 ml of 0.100 m NaOH, constant pressure, calorimeter, heat capacity, same as 125g of water, temperature rises, energy required.