Question

If 80,000 Joules of heat is absorbed by 210 grams of ice at 0°C, what happens to the ice?

It partially melts and stays at 0°C
It completely melts but stays at 0°C
It completely melts and has a final temperature of 11.2°C
It completely melts and has a final temperature of 22.4°C
It completely melts and has a final temperature of 33.6°C

Answer 1

It completely melts and has a final temperature of 22.4°C

Step-by-step explanation:

(I am very bad at explaining, I am not a teacher, I am a student but I had exact same question on my test so I wanted to help.)

Okay, well to find the Heat required to melt Ice, we have to use the equation:

Q=(m·cΔT)+(m·hf)

• Q= Heat

• M= Mass

• C= Specific heat

• ΔT= Change in temperature.

• hf= heat fusion

So we can just plug in the values into the equation and see which one adds up too 80,000. (there is probably a better way i just did it this way)

For this situation, we know that:

• Mass=210 grams

• Specific heat = 2.10 (I got this number 2.10 from the internet. The universal number for specific heat of ice is 2.10 J/g°C )

• Change in temperature= 0 °C or 11.2 °C or 22.4 °C or 33.6 °C (all the answers)
• Heat fusion=334 (universal number for heat fusion of melting ice is 334)

So we can just change the value of change and temperature and see which one equals 80,000.( I will bold the value of change in temperature.)

Q=(m·cΔT)+(m·hf)

1. (210g)*(2.10)*(0)+(210)*(334)=70140
2. (210g)*(2.10)*(11.2)+(210)*(334)=75079.2
3. (210g)*(2.10)*(22.4)+(210)*(334)=80018.4
4. (210g)*(2.10)*(33.6)+(210)*(334)=84957.6

So which one equals 80,000? Equation #3 with the temperature at 22.4 °C

So the answer would be It completely melts and has a final temperature of 22.4°C.

Hope this makes sense, again I am not a teacher I am so bad at explaining, but I did my best. ;)