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?
Use q equals m C subscript p Delta T..

A). 4.62 kJ
B). 10.0 kJ
C). 14.7 kJ
D). 38.5 kJ

Answer 1

Answer:

4.62 kJ of heat is given off in the reaction.

Explanation:

Let's assume specific heat of calorimeter is negligible.

So, amount of heat given off, q = heat absorbed by solution

                                                    = ($m_{solution}\times C_{solution}\times \Delta T_{solution}$)

where, m is mass, C is specific heat and $\Delta T$ is change in temperature.

So, q = $[120.0g\times 4.184\frac{J}{g.^{0}\textrm{C}}\times (29.20-20.00)^{0}\textrm{C}]$

         = 4619 J

         = 4.62 kJ (3 sig. fig.)

Option (A) is correct

         

Answer 2

Answer:

A

Explanation:

4.62 kJ

just took test on edge!!