Question

When 40.0 mL of 1.00 M H2SO4 is added to 80.0 mL of 1.00 M NaOH at 20.00°C in a coffee cup calorimeter, the temperature of the aqueous solution increases to 29.20°C. If the mass of the solution is 120.0 g and the specific heat of the calorimeter and solution is 4.184 J/g • °C, how much heat is given off in the reaction? (Ignore the mass of the calorimeter in the calculation.)

Use q equals m C subscript p Delta T..
4.62 kJ
10.0 kJ
14.7 kJ
38.5 kJ

Answer 1

4.62 kJ

Step-by-step explanation:

The heat given off in the reaction is equal to the heat absorbed by the solution. We can use the following equation to calculate the heat absorbed by the solution:

q = m * C * ΔT

where:

• q is the heat absorbed (in J)
• m is the mass of the solution (in g)
• C is the specific heat of the solution (in J/g • °C)
• ΔT is the change in temperature (in °C)

In this case, we have:

m = 120.0 g

C = 4.184 J/g • °C

ΔT = 29.20°C - 20.00°C = 9.20°C

Therefore, the heat absorbed by the solution is:

q = 120.0 g * 4.184 J/g • °C * 9.20°C = 4.619 kJ

Since the heat given off in the reaction is equal to the heat absorbed by the solution, the heat given off in the reaction is also 4.619 kJ.

Therefore, the answer is 4.62 kJ.

Answer 2

Solution :- Given data mass of solution = 120 g specific heat

Step-by-step explanation: