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 going to be mutualism cuz they both benefit from the relationship.

~batmans wife dun dun

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.