Question

Calculate the amount of heat required to raise the temperature of a 65-g sample of water from 32∘C to 65∘C. (The specific heat capacity of copper is 4.184 J/g∘C.)

Q=M*C*delta T
65g*4.184*(65-32)
89.7 J

Answer 1

I didn't check the math but the numbers and substitution are correct.

Answer 2

Calculate the amount of heat required to raise the temperature of a 65-g sample of water from 32 ∘C to 65 ∘C. (The specific heat capacity of water is 4.184 J/(g⋅∘C).)

The answer is = 9.0 * 10cube J

Answer 3

[AI-generated answer — Clown Bot]

Well, don't get all hot and bothered, but I have a little joke for you. Why did the scarecrow become a successful comedian? Because he was outstanding in his field! Now let's talk about that heat calculation.

You're on the right track with the formula Q = m * C * ΔT. Let's plug in the values:

Q = 65 g * 4.184 J/g∘C * (65∘C - 32∘C)

Now let's simplify:

Q = 65 g * 4.184 J/g∘C * 33∘C

Q = 89.7 J

So the amount of heat required to raise the temperature of the water is "hot off the press" at 89.7 J. Be careful not to get burned!

Answer 4

[AI-generated answer — Explain Bot]

To calculate the amount of heat required to raise the temperature of a substance, you can use the formula Q = m * c * ΔT, where Q is the amount of heat, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.

In this case, you have a 65-gram sample of water and need to calculate the amount of heat required to raise its temperature from 32∘C to 65∘C. The specific heat capacity of water is approximately 4.184 J/g∘C.

Substituting the values into the formula, you get:

Q = (65 g) * (4.184 J/g∘C) * (65∘C - 32∘C)

Simplifying the equation:

Q = 65 g * 4.184 J/g∘C * 33∘C

Q = 89.7 J

Therefore, the amount of heat required to raise the temperature of the 65-g sample of water from 32∘C to 65∘C is 89.7 Joules.