which of the following substances (with specific heat provided) would show the greatest temperature change upon absorbing 100.0 J of heat?
See below.
To determine which substance would show the greatest temperature change upon absorbing 100.0 J of heat, we need to use the equation:
Q = m * c * ΔT
where:
Q is the amount of heat energy absorbed or released (in joules),
m is the mass of the substance (in grams or kilograms),
c is the specific heat capacity of the substance (in J/g°C or J/kg°C),
ΔT is the change in temperature (in °C).
We are given the amount of heat energy, Q, as 100.0 J. The mass, m, is not provided for any substances, so we cannot make a comparison based on mass. However, we are given the specific heat capacities for the substances.
Let's compare the specific heat capacities of the given substances to determine which substance would exhibit the greatest temperature change:
Substance A: Specific heat = 0.5 J/g°C
Substance B: Specific heat = 0.2 J/g°C
Substance C: Specific heat = 1.0 J/g°C
Substance D: Specific heat = 0.8 J/g°C
From the provided values, we can see that Substance C has the highest specific heat capacity of 1.0 J/g°C. According to the equation, substances with a higher specific heat capacity require more heat energy to increase their temperature compared to substances with lower specific heat capacities.
Therefore, Substance C would show the smallest temperature change since it would require the greatest amount of heat energy (Q) to produce a temperature change. Conversely, Substance B would show the greatest temperature change as it has the lowest specific heat capacity.
So, based on the given specific heat capacities, Substance B would show the greatest temperature change upon absorbing 100.0 J of heat.