Substance A has a specific heat of .650J/gK and substance B has a specific heat of .325J/gK. If 100 J of energy is applied to a 10 g sample of each substance, which will have a higher temperature?
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To determine which substance will have a higher temperature, we need to compare the amount of energy transferred to each substance. The formula to calculate energy transferred is:
Energy (Q) = mass (m) × specific heat (c) × change in temperature (ΔT)
Let's calculate the change in temperature for each substance.
For Substance A:
Q = 100 J (given)
m = 10 g (given)
c = 0.650 J/gK (given)
Using the formula, we can rearrange it to solve for ΔT:
ΔT = Q / (m × c)
ΔT = 100 J / (10 g × 0.650 J/gK)
ΔT = 15.38 K
For Substance B:
Q = 100 J (given)
m = 10 g (given)
c = 0.325 J/gK (given)
Using the same formula:
ΔT = Q / (m × c)
ΔT = 100 J / (10 g × 0.325 J/gK)
ΔT = 30.77 K
Comparing the change in temperature, we can see that Substance B has a larger change in temperature (30.77 K) compared to Substance A (15.38 K). Therefore, Substance B will have a higher temperature after the energy transfer.