Calculate the amount of heat needed to raise the temperature of 358g of ice from -24.5degreesC to 456degreesC.

Question

greatlife44 · Answer

@Clemsongator Do you know how to approach this?

anonymous · Answer

i got the amount of energy to cget it to 0C as 18419.1J
but idk where to go from there

greatlife44 · Answer

alright. 

The amount of heat released q is equal to the mass of the substance in grams, times C the specific heat times delta T the temperature change. 

$$q = m~C~\Delta~T$$

anonymous · Answer

yeah

greatlife44 · Answer

Our final temperature is 45.6 degrees C right?

anonymous · Answer

456 degrees C

greatlife44 · Answer

Well, I guess I decided to find the specific heat of ice. how much energy we need to put into ice to melt it. we can't do our calculation without it.  

458*C is a pretty high temperature so that's why i'm asking.  

$$2.65~ J/grams*K$$ specific heat of ice 

K means temperature in kelvins. so we convert our temperatures to kelvins, 

$$C^{0}+273 = Kelvins$$

$$-24.5+273 = 248.5 K_{T_{1}}$$

$$273+456 = 729K_{T_{2}}$$

then we put everything into this formula 

alright. 


$$q = m~C~\Delta~T$$

$$q = (358g)(2.65 \frac{ J }{ grams*K })*(729_{t2}-248.5_{t1})K  = 456~Kilo~Joules$$

anonymous · Answer

i thought the specific heat of ice was 2.1

greatlife44 · Answer

The values are different depending on what units you choose to use @Clemsongator