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