When 10.g of ch3cooh is combusted in a sealed calorimeter, it releases enough energy to heat 2000. g of water from 23.5 °c to 34.3 °c. a. calculate the energy released per 10 g of ch3cooh. b. calculate the energy released per mole of ch3cooh.

a. 90.288 kJ.

b. - 54.06 kJ/mol.

Explanation:

a. Calculate the energy released per 10 g of CH₃COOH.

Q = m.c.ΔT,

where, Q is the amount of heat released to water (Q = ??? J).

m is the mass of water (m = 2000.0 g).

c is the specific heat capacity of solution (c = 4.18 J/g.°C).

ΔT is the difference in T (ΔT = final temperature - initial temperature = 34.3°C - 23.5°C = 10.8°C).

∴ Q = m.c.ΔT = (2000.0 g)(4.18 J/g.°C)(10.8°C) = 90288 J = 90.288 kJ.

b. Calculate the energy released per mole of CH₃COOH.

∵ ΔH = Q/n

no. of moles of CH₃COOH (n) = mass/atomic mass = (10.0 g)/((60.052 g/mol) = 0.167 mol.

∴ ΔH = - Q/n = - (90.288 kJ)/(0.167 mol) = - 54.06 kJ/mol.

The negative sign is not from calculation, but it is an indication that the reaction is exothermic.

its first and third is your answer i did the qustion the fourth isnt right

it should have an internal chamber and two thermometers sticking out of the top. the internal chamber will also be closed off from the outside.