(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

a 0.20kg lead shot is heated to 90 degrees celsius and dropped into an ideal calorimeter containing 0.50kg of water initially at 20 degrees celsius. What is the final equilibrium temperature of the lead shot? The specific heat capacity of lead is 128 Joules/(kg degrees celsius) and the specific heat capacity of water is 4186Joules/(kg degrees Celsius)

Ml = 0.20

Cl = 128

Til = 90

Mw = 0.50

Cw = 4186

Tiw = 20

2. Relevant equations

Q= mass x heat capacity x difference in temperature

Qabsorbed + Qreleased = 0

3. The attempt at a solution

0.20 x 128 x (T2 - 90) + 0.50 x 4186 x(T2 - 20)

25.6 x (t2 -90) + 2093 x (T2-20)

I am completely stuck after this. I don't know what to do with the difference in temperature part. I've looked at example equations and it shows the temperature given getting transformed into joules? So in this equation the 90 and 20 would be replaced by different numbers with the unit Joules after. I don't understand why this is happening. Thank you for any help and I appreciate you taking the time to read this.

This may not be very clear, so if I need to explain more please let me know

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# Grade 11 Heat Capacity question

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