In my class, we've started thermodynamics and I think I'm having trouble understanding the equation to calculate heat transfer (

q = mC_{p}ΔT ). I've supplied the problem below as well as my work. I was just wondering if someone on here would mind checking my work.

Question: How much heat is required to raise the temperature of 754 g of water from 32.9°C to 88.6°C?

Mathematical Answer:

q = 754(4.184J/g°C)55.7°C

q = (754)(4.184)

q = (3,154.746)(55.7)

q = 175,718.7952J

My answer is 175,718.7952 joules.

Textual Answer

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I first identified my 'm', the mass of the water at 754 grams. Then, I identified the specific heat capacity of water, which is 4.184. After I identified both the mass of the water and the heat capacity of water, I found the difference between my two temperatures, which will give me a positive 'q' value in the end. The difference between my two temperatures, 32.9°C and 88.6°C was 55.7°C. I plugged in all of my numbers into the equation ( q = mC_{p}ΔT ) and multiplied from left to right. My final answer was 175,718.7952 joules.

Thank you for reading and for your time!