My teacher provided info about a worksheet of problems.
Special Heat of water: 4.184
Special Heat of Steam: 2.09
Special Heat of Ice: 1.8

Based on this info, and the notes we have taken on phase changes, we are supposed to find out how much energy is needed to change certain substances.

I thought, however, that in order to create a phase change, one must use the q=m,delta,Hfusion or m,delta,Hvap. How can I perform these equations without the Hvap/fusion info provided?!

...60g of water at 43 degrees celcius to steam at 140 degrees celcius.

1. 👍
2. 👎
3. 👁
1. q1 = heat to move T of water from 43 C to 100 = mass x speicif heat liquid water x (
Tf - Ti). Tf is final T (in this case 100 and Ti is initial T (in this case 43 C.)
Then you DO, definitely, need the delta H vap for water.
q2 = heat to evaporate water = mass x delta Hvap

q3 = heat to move T of steam from 100 C to 140 C = mass x specific heat steam x (Tf - Ti) =
The total is q1 + q2 + q3.

Judging from your post, I think you knew all of this. You will need to either look up delta Hvap or ask your teacher tomorrow. By the way, note the correct spelling of Celsius.

1. 👍
2. 👎

## Similar Questions

1. ### chemistry

1. Given that 50 grams of ice is heated at -20.0 °C to steam at 135.0 °C. i. Show the graph of the changes from ice to steam ii. Calculate the energy needed to change the ice to steam Please use these values: Heat of fusion =

2. ### chem

Calculate the amount of heat required to raise the temperature of a 65-g sample of water from 32∘C to 65∘C. (The specific heat capacity of copper is 4.184 J/g∘C.) Q=M*C*delta T 65g*4.184*(65-32) 89.7 J

3. ### Chemistry

Calculate the amount of heat (in calories) required to raise the temperature of 200g of water from 20C to 50C. The specific heat of water is 1.00 cal/g. I have done other spacific heat problems but on this one i don't know how to

4. ### Chemistry

How much heat is required to warm 122g of water by 23.0°C? Specific heat is 4.184 J/g° C. Please show work:(((

1. ### chemistry

KCl(s) → K+(aq) + Cl‾ (aq) Solid KCl dissolves as shown in the above equation. A 6.60 g sample of KCl was dissolved in 42.3 g of water. The initial temperature of the water was 21.90°C. After the compound dissolved, the

2. ### Chemistry

The heat capacity of liquid water is 4.18 J/g•C and the heat of vaporization is 40.7 kJ/mol. How many kilojoules of heat must be provided to convert 1.00 g of liquid water at 67C into 1.00 g of steam at 100C? A. 22.7 kJ

3. ### Chemistry

A piece of copper metal is initially at 100.0°C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0°C. After stirring, the final temperature of both copper and water is 25.0°C.

4. ### Chemistry

Calculate the heat released when 64.5g of steam at 119 C is converted to water at 36 C. Assume the specific heat is 4.184 J/g*C for water, the specific heat of steam is 1.99J/g*C, and the heat of vaporization is 40.79 kJ/mol for

1. ### Chemistry

For a 8.88 gram sample of ice at -43.6°C , what is the minimum amount of heat (in kJ) needed to convert the sample to liquid water at 0.00°C? Physical data for water: specific heat (ice) = 2.10 J/g°C specific heat (water) =

2. ### Chemistry - Heat of Fusion of Ice

Conclusion question(s) from a lab we did to find the heat of fusion of ice: Does the value obtained for the molar heat of fusion depend on the volume of water used? Does it depend on the mass of ice melted? Does it depend on the

3. ### Chemistry

How many kJ of heat are required to convert 1.00 g of ice at -25°C to steam at 125°C? s(ice) = 2.108 J/g·°C s(liquid water) = 4.184 J/g·°C s(steam) = 1.996 J/g·°C heat of fusion = 6.01 kJ/mol heat of vaporization = 40.79

4. ### Chemistry

To begin the experiment, 1.65g of methane CH is burned in a bomb calorimeter containing 1000 grams of water. The initial temperature of water is 18.98°C. The specific heat of water is 4.184 J/g °C. The heat capacity of the