A community for students.
Here's the question you clicked on:
 0 viewing
anonymous
 4 years ago
a neutralization reaction occurs when 120ml of 1.00mol/l lioh and 160nl of 0.75 mol/l hno3 are mixed in an insulated cup. initially, the solutiona are at the same temperature. If the highest temp during mixing was 24.5C, what was the iniyial temp of the solutions? The density is 1.00g/ml and the specific heat capacity is 4.19J/gC.
anonymous
 4 years ago
a neutralization reaction occurs when 120ml of 1.00mol/l lioh and 160nl of 0.75 mol/l hno3 are mixed in an insulated cup. initially, the solutiona are at the same temperature. If the highest temp during mixing was 24.5C, what was the iniyial temp of the solutions? The density is 1.00g/ml and the specific heat capacity is 4.19J/gC.

This Question is Closed

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Vt=280mL m=280g \[DeltaH=53.1kJ\] n=0.12mol Ti=(Q/mc) Tf This is all I got so far.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0LiOH+HNO3> LiNO3 + H2O+ 53.1kJ

Rogue
 4 years ago
Best ResponseYou've already chosen the best response.1Is that the whole question? It seems a bit vague. :( How did you get the delta H by the way?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Yeah that is the question. This equation was given LiOH+HNO3> LiNO3 + H2O+ 53.1kJ.

Rogue
 4 years ago
Best ResponseYou've already chosen the best response.1Oh, okay, how about the mass 280 g?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0so i calculated the total volume and then i used the density formula to find the total mass.

Rogue
 4 years ago
Best ResponseYou've already chosen the best response.1Hmm, I feel like the problem is a bit more complicated than this, but why don't you just try substituting what you?\[T _{i}^{} = \frac {Q}{mc}  T _{f}^{} = \frac {53 kJ}{280 g * 0.00419 J/gC}  24.5 C\]

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0my teach told me to use deltaHr =deltaH/n

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0so I first found the n=mv=1.00mol/L * 0.12L=0.12mol

Rogue
 4 years ago
Best ResponseYou've already chosen the best response.1Ah, right, 53.0 kJ of energy is released for every 1 mole of LiNO3 formed. So the actual delta H for the sample given would be 53.0 kJ/mol * 0.12 mol = 6.36 kJ

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0but it is in kJ not kJ/mol :S I'm confused.

Rogue
 4 years ago
Best ResponseYou've already chosen the best response.1Well, according to the reaction, when 1 mole is formed when 53.0 kJ is released. So the delta H rxn = 53.0 kJ/mol.

Rogue
 4 years ago
Best ResponseYou've already chosen the best response.1Hmm, am I explaining that or just repeating? Don't really know how to say it...

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Oh okay, now it makes sense :) Thank you soooo much. Let me calculate the final answer and show it to you.

Rogue
 4 years ago
Best ResponseYou've already chosen the best response.1The Q should be negative right?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0I would guess so, since energy is released. right? then the answer would be 29.9

Rogue
 4 years ago
Best ResponseYou've already chosen the best response.1I really don't like this question :( It'd be great if someone else could also do this question to verify the answer.
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.