Ask Questions, Get Answers

Want to ask us a question? Click here
Browse Questions
0 votes

How much heat would release when an aqueous solution containing 0.5 mol of $HNO_3$ is mixed with 0.3 mol of $OH^{-1}$? Given, enthalpy of neutralisation is -57.1 kJ.

(a) 28.5 kJ
(b) 17.1 kJ
(c) 1.7 kJ
(d) 2.85 kJ
Can you answer this question?

1 Answer

0 votes
Answer: 17.1 kJ
0.5 mol $HNO_3 \equiv$ 0.5 mol $H^+$
$H^+ + OH^- \longrightarrow H_2O$ ; $\Delta H = -57.1$ kJ
Here, $OH^-$ = 0.3 mol
Thus, $OH^-$ is the limiting reactant.
When 1 mol of $OH^-$ ions are neutralised heat released = 57.1 kJ
0.3 mol of $OH^-$ ions are neutralised heat relaesed $= 57.1 \times 0.3$ = 17.13 kJ
answered Feb 26, 2014 by mosymeow_1

Related questions

Ask Question
student study plans
JEE MAIN, CBSE, NEET Mobile and Tablet App
The ultimate mobile app to help you crack your examinations
Get the Android App