A community for students.
Here's the question you clicked on:
 0 viewing
bak11
 2 years ago
An ice cube has mass 9.0g and is added to a cup of coffee. The coffee's intial temp. is 90.0 deg. Celsius and the cup contains 120.0 g of liquid. Assume the specific heat capacity of coffee is the same as that of water. The heat of fusion of ice (associated with ice melting) is 6.0kJ/mol. Find the temp. of coffee after ice melts.
How do we get rid of the /mol under the kJ?
Also, may I get a hint please?
bak11
 2 years ago
An ice cube has mass 9.0g and is added to a cup of coffee. The coffee's intial temp. is 90.0 deg. Celsius and the cup contains 120.0 g of liquid. Assume the specific heat capacity of coffee is the same as that of water. The heat of fusion of ice (associated with ice melting) is 6.0kJ/mol. Find the temp. of coffee after ice melts. How do we get rid of the /mol under the kJ? Also, may I get a hint please?

This Question is Closed

benjaminf
 2 years ago
Best ResponseYou've already chosen the best response.0So water has molar mass 18 g/mol and you have an ice cube of 9.0 g, that looks like half a mole of ice. The heat of fusion of ice is 6.0 kJ/mol and you have 0.5 moles of ice, so the energy used to melt your ice cube is 3.0 kJ That answers the first part of your question, the next thing to do is to take the specific heat capacity of water and figure out how much those 3.0 kJ are going to change the overall temperature of the (129.0g) of coffee. Hope that helps.
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.