Question

Chemistry. Please some 1 help.
Calculate the heat needed at 0 Celsius to make each of the following changes of state. Indicate whether heat was absorbed or released.
a. calories to melt 65g of ice
b. calories to melt 17g of ice
c kilocalories to freeze 225 g of water

Answer 1

Q = mL

Answer 2

Heat=mass*heat of vaporization
540cal/1gm water=heat of vaporization

Answer 3

a calorie is the amount of heat needed to raise the degree of 1 gram of water by 1, so to melt 65g of ice at 0 degrees C, you would need 65 calories.

Answer 4

So what's the answer to A. B. C. or possible answers? and how you got to them any suggestions?

Answer 5

r u crazy dylan?

Answer 6

a. 65 x 334 J (absorbed)
b. 17 x 334 J (absorbed)
c. 225 x 334 J (released)

Answer 7

get it?

Answer 8

No I don't get it. Since the correct answers from the book should be.
a. 5200 cal (absorbed)
b. 1400cal (absorbed)
c. 18kcal (released)
And i don't get it how they got these answers.

Answer 9

b. should be 1360 and not 1400

Answer 10

the latent heat of fusion of water is 80 cal/gm

Answer 11

see heat = mass x latent heat

Answer 12

so a is
65 x 80 cal

Answer 13

now?

Answer 14

b is 1400 because of sig figs. i assume you know what that is.

Answer 15

yes

Answer 16

then dont wirte it 1400 instead u can write 1.4 x 10^2

Answer 17

which is the same as 1400.
can you explain where you got the numbers to calculate. abc ? i'm looking and not seeing it. i don't get it. just yet.