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.)

Answer 1

Approximately 384.64 J of heat is given off in the reaction.

Step-by-step explanation:

The heat produced by a reaction can be found using the equation: q = mcΔT, where q is the heat, m is the mass, c is the specific heat, and ΔT is the change in temperature.

In this case, the heat given off by the reaction is equal to the heat absorbed by the solution. We can calculate the heat absorbed by the solution using the equation q(solution) = m(solution) * c(solution) * ΔT(solution).

Assuming the specific heat of the solution is the same as the specific heat of pure water (4.184 J/g • °C), we can plug in the values: q(solution)

= 120.0 g * 4.184 J/g • °C * (29.20 °C - 20.00 °C)

= 384.64 J.

Therefore, approximately 384.64 J of heat is given off in the reaction.

Answer 2

I just took the test, the answer is A. 4.62 kJ