The specific heat of silver is 0.057 calories/gram°C. If 10.0 grams of silver were heated and the temperature of the sample changed by 20.0°C, how many calories of heat energy were absorbed by the sample?
(A)3,508 calories
(B)0.029 calories
(C)11.4 calories
(D)0.114 calories
(d) 0.114
The answer would be (D) because you have to multiply the 20.0C to 0.057 and that will get you 1.14 than you divide it by the 10 grams and you should get 0.114 or .114
3,508
The specific heat of gold is 0.031 calories/gram°C. If 10.0 grams of gold were heated and the temperature of the sample changed by 20.0°C, how many calories of heat energy were absorbed by the sample?
To find the amount of heat energy absorbed by the sample, we can use the equation:
Q = m * c * ΔT
Where:
Q = heat energy absorbed by the sample
m = mass of the sample in grams (10.0 grams)
c = specific heat of silver in calories/gram°C (0.057 calories/gram°C)
ΔT = change in temperature (20.0°C)
Let's substitute the given values into the equation:
Q = 10.0 grams * 0.057 calories/gram°C * 20.0°C
Now, we can calculate the answer:
Q = 11.4 calories
Therefore, the amount of heat energy absorbed by the sample is 11.4 calories.
The correct answer is (C) 11.4 calories.