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.)

4.62 kJ

4.62kj

To calculate the heat given off in the reaction, you can use the formula:

q = mcΔT

Where:
q is the heat given off,
m is the mass of the solution,
c is the specific heat of the calorimeter and solution, and
ΔT is the change in temperature.

First, you need to calculate the change in temperature (ΔT). To do this, subtract the initial temperature from the final temperature:

ΔT = Tf - Ti
ΔT = 29.20°C - 20.00°C
ΔT = 9.20°C

Next, substitute the values into the formula and calculate the heat (q):

q = (m)(c)(ΔT)
q = (120.0 g)(4.184 J/g • °C)(9.20°C)
q = 4,620 J

Finally, convert the answer to kilojoules:

q = 4,620 J ÷ 1000
q = 4.62 kJ

Therefore, the heat given off in the reaction is 4.62 kJ.

q = mass x specific heat x (Tfinal-Tinitial)

q = 120g x 4.184 J/g*C x (29.2-20)
q = ?

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Figure It Out Your Own Damn Self.