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

A

Step-by-step explanation:

4.62 kJ

just took test on edge!!

Answer 2

4.62 kJ of heat is given off in the reaction.

Step-by-step explanation:

Let's assume specific heat of calorimeter is negligible.

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

= (
`m_(solution)* C_(solution)* \Delta T_(solution)`)

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

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

= 4619 J

= 4.62 kJ (3 sig. fig.)

Option (A) is correct