Answer to Question #97594 in General Chemistry for Brittany Wallace

Question #97594
1. You mix 45 mL of 0.20 M HCl with 55 mL of 0.20 M KOH in a perfectly insulated solution calorimeter. The following reaction occurs:
HCl(aq) + KOH(aq) KCl(aq) + H2O(l)
The temperature of both solutions before mixing is 20.50 °C. The temperature of the solution rises to 21.69 °C after mixing. What is the enthalpy change per mole of water produced? The specific heat capacity of water and the solution is 4.2 J/g·K. Assume the density of all solutions is 1.00 g/mL.
1
Expert's answer
2019-10-31T07:29:57-0400

HCl(aq) + KOH(aq) --------> KCl(aq) + H2O(l)

45 ml 55ml

0.2 molar 0.2 molar

0.2 × 45/1000 0.2 ×55/1000

0 0.2 ×10/1000 0.2×45/1000 0.2×45/10^3

Volume of the solution is 100 ml.

Density of the solution is 1gm/ml.

Mass of the solution(m) is 100gm.

"C=4.2J\/g.K"

"Tf=294.69 K"

"Ti =293.5 K"

"Qabs by solution = m\u00d7C\u00d7change in T"

"Qabs by solution = 100g \u00d74.2J\/g.K\u00d71.19K"

"Qabs by solution = 499.8 J"

"Qreaction = -Qabs by solution=-499.8J"

"enthalpy change\/mole of water =Qreact\/moles"

"enthalpy change= -499.8 J\/(0.2\u00d745\/1000)mol"

"enthalpy change= - 55.53\u00d7 10^3 J\/mol"

"enthalpy change= -55.53KJ\/mol" (Ans)




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