The heat evolved, q, in a reaction of 0.10 mol HCl(aq) with excess NaOH(aq) is 96 calories.
a. Calculate the number of Joules that is evolved.
b. Calculate the number of kJ/mol HCl.
c. Is the reaction exothermic or endothermic?
d. What is ΔrH for the reaction in kJ/mol·rxn with the correct sign?
Please, show work. I want know how to do these problems.
Thank you!
Chemistry help, thermodynamics?
2018-01-26 8:23 am
回答 (2)
2018-01-26 10:21 am
✔ 最佳答案
a.1 J = 4.184 cal
Number of joules = (96 cal) × (1 J / 4.184 cal) = 23 J (to 2 sig. fig.)
b.
(23/1000 kJ) / (0.10 mol HCl) = 0.23 kJ/mol HCl
c.
The reaction is exothermic.
This is because heat is evolved.
d.
HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l) …… ΔrH = -0.23 kJ
2018-01-26 9:23 am
1 cal = 4.181 J
a) calculate J from cal
b) 0.10 mol gives answer a) J
so 1 mol gives answer a)/0.1 J/mol
c) heat is released so final energy less than started and deltaH must be .....
d) if .... c) the the sign of deltaH is ....
a) calculate J from cal
b) 0.10 mol gives answer a) J
so 1 mol gives answer a)/0.1 J/mol
c) heat is released so final energy less than started and deltaH must be .....
d) if .... c) the the sign of deltaH is ....
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