Asked by Mellisa
If 0.120 moles of water are produced in the reaction
H+(aq)+OH-(aq)-->H2O(l)
delta H=-56.2 kJ/mol
I have tried this problem a ton of times and aris keeps telling me I'm incorrect. Can you please help me with solving this problem
H+(aq)+OH-(aq)-->H2O(l)
delta H=-56.2 kJ/mol
I have tried this problem a ton of times and aris keeps telling me I'm incorrect. Can you please help me with solving this problem
Answers
Answered by
DrBob222
Am I missing something?
First, what's the question? Is it to calculate the heat released by the reaction? Or is it something else?
56.2 kJ/mol x 0.120 mol = 6.744 kJ which rounds to 6.74 kJ to three significant figures (s.f.). I OFTEN find that when students are keying answers into a data base that the problem is incorrect number of s.f.
First, what's the question? Is it to calculate the heat released by the reaction? Or is it something else?
56.2 kJ/mol x 0.120 mol = 6.744 kJ which rounds to 6.74 kJ to three significant figures (s.f.). I OFTEN find that when students are keying answers into a data base that the problem is incorrect number of s.f.
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