# Chemistry

A quantity of ice at 0.0 degrees C was added to 33.6 of water at 21.0 degree C to give water at 0.0 degrees C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g * degrees C)

q = mass x specific heat x delta T?
q = mass x heat fusion?

I don't understand what to plug in
and where

Heat removed from water in going from 21.0 to zero C is
mass x specific heat x delta T.
mass = 33.6 g
specific heat is 4.184 J/g*K
delta T is 21.0 - 0.

heat added to ice to melt it is
mass x heat fusion.
mass is the unknown.
heat fusion is given.
Note: you need to work in the same units. The heat of fusion is quoted in the problem in kJ/mol but I quoted the specific heat of water in J/gram. One needs to be changed. I would suggest the 4.184 be changed.

ok so i did 33.6g (4.184 J/g)(21.0-0)
So how do i get J to kJ/mol

1. 👍 0
2. 👎 0
3. 👁 727
1. The specific heat of water in J/mol = 75.3. You can change 33.6 g water to mols by 33.6/18 = ??
Then (33.6/18)*75.3*21 = ?? Joules.
You can change to kJ by ??/1000 = xx.

1. 👍 0
2. 👎 0

## Similar Questions

1. ### Science

A 40.0 g block of ice at -15 degrees C is dropped into a calorimeter (of negligible heat capacity) containing water at 15 degrees C. When equilibrium is reached, the final temperature is 8.0 degrees C. How much water did the

asked by Ciara on November 29, 2014
2. ### chemistry

The enthalpy of fusion of ice is 6.020 kJ/mol. The heat capacity of liquid water is 75.4 J/mol degrees Celsius. What is the smallest number of ice cubes at 0 degrees Celsius, each containing one mole of water, necessary to cool

asked by maath on January 28, 2019
3. ### Chemistry

Given that the specific heat capacities of ice and steam are 2.06 J/g degrees C and 2.03 J/g degrees C, respectively, calculate the total quantity of heat evolved when 10.0 g of steam at 200 degrees C is condensed, cooled, and

asked by Joe Schmo on April 27, 2011
4. ### Chemistry

How much ice (in grams) be added to lower the temperature of 355 mL of water from 25 ∘C to 5 ∘C ? (Assume the following: the density of water is 1.0 g/mL, the ice is at 0 ∘C, the heat of fusion of ice is 6.02 kJ/mol, and the

asked by Anonymous on January 19, 2017
5. ### Chem; States of Matter

To an insulated container with 100.0 g H2O (l) at 20.0 degrees C, 175 g steam at 100.0 degrees C and 1.65 kg of ice at 0.0 degrees C are added. a) What mass of ice remains unmelted after equilibrium is reached? b) what additional

asked by K on February 11, 2014
1. ### Physics

A 100g piece of ice at 0 degrees celcius is placed into a container holding 200g of water, initially at temperature 25 degrees celcius. Heat flows from the water to the ice, cooling the water and melting the ice. Calculate a) how

asked by Betty on November 4, 2015

If 10-kg of ice at 0 degrees Celsius is added to 2-kg of steam at 100 degrees Celsius, the temperature of the resulting mixture is? Use Joules. ANSWER: 40 Specific Heats: Ice = 2060 Steam = 2020 Latent Heats: Water melting =

asked by Max on February 11, 2013
3. ### physics

A 40-g block of ice is cooled to −71°C and is then added to 590 g of water in an 80-g copper calorimeter at a temperature of 27°C. Determine the final temperature of the system consisting of the ice, water, and calorimeter.

asked by anthony on April 11, 2012
4. ### Chemistry

Suppose that 100.0 g of ice a 0 degreesC are added to 300.0 g of water at 25.0 degrees . Is this sufficient ice to lower the temperature of water to 5.00 degrees C and still have ice remaining? Calculate the energy (heat) which

asked by Sage on February 24, 2016
5. ### physics

Given: latent heat of fusion of water 3.33x10^5 J/kg. A 147 g cube of ice at 0 degress C is dropped into 1.3 kg of water that was originally at 79 degrees C. What is the final temperature of the water after the ice melts.

asked by Ericka on December 8, 2009