Look at the chart below.
Metal Specific heat (J/g°C)
Calcium (Ca) 0.647
Iron (Fe) 0.449
Silver (Ag) 0.235
Gold (Au) 0.129
If the same amount of heat is added to 25.0 g samples of each of the metals in the chart, which metal will experience the largest temperature change?
A
Ca
B
Fe
C
Ag
D
Au
To determine which metal will experience the largest temperature change, we need to compare the specific heat of each metal. The metal with the lowest specific heat will experience the greatest temperature change.
Looking at the chart, we can see that gold (Au) has the lowest specific heat at 0.129 J/g°C. Therefore, the metal that will experience the largest temperature change when the same amount of heat is added is gold (Au).
Therefore, the answer is D) Au.
To determine which metal will experience the largest temperature change when the same amount of heat is added, we need to compare the specific heat values of the metals. Specific heat is a measure of how much heat energy is required to raise the temperature of a given mass of a substance by a certain amount.
The formula to calculate the temperature change is as follows:
Temperature change (ΔT) = Heat energy (Q) / (Mass (m) * Specific heat (C))
Since the same amount of heat is added to each metal (Q is constant), we can ignore it for comparison purposes.
Let's calculate the temperature change for each metal using the given formula:
For Calcium (Ca):
ΔT = Q / (m * C) = Q / (25.0 g * 0.647 J/g°C)
For Iron (Fe):
ΔT = Q / (m * C) = Q / (25.0 g * 0.449 J/g°C)
For Silver (Ag):
ΔT = Q / (m * C) = Q / (25.0 g * 0.235 J/g°C)
For Gold (Au):
ΔT = Q / (m * C) = Q / (25.0 g * 0.129 J/g°C)
Comparing the specific heat values, we can conclude that the metal with the lowest specific heat value will experience the largest temperature change when the same amount of heat is added. Therefore, the correct answer is:
D) Au (Gold) with a specific heat of 0.129 J/g°C.
To determine which metal will experience the largest temperature change, we need to compare the specific heat values of the metals.
The specific heat of a substance is the amount of heat energy required to raise the temperature of one gram of the substance by one degree Celsius.
We are given the specific heat values for each metal:
- Calcium (Ca): 0.647 J/g°C
- Iron (Fe): 0.449 J/g°C
- Silver (Ag): 0.235 J/g°C
- Gold (Au): 0.129 J/g°C
The formula to calculate the amount of heat energy absorbed or released by a substance is:
Heat energy = mass × specific heat × temperature change
Since the mass is the same (25.0 g) and the heat energy added is the same, we can compare the temperature change for each metal.
Using the formula, we can rearrange it to calculate the temperature change:
Temperature change = Heat energy / (mass × specific heat)
For each metal, plugging in the values:
- Calcium (Ca): Temperature change = Heat energy / (25.0 g × 0.647 J/g°C)
- Iron (Fe): Temperature change = Heat energy / (25.0 g × 0.449 J/g°C)
- Silver (Ag): Temperature change = Heat energy / (25.0 g × 0.235 J/g°C)
- Gold (Au): Temperature change = Heat energy / (25.0 g × 0.129 J/g°C)
Since the heat energy and mass are constant, the metal with the smallest specific heat will experience the largest temperature change. Looking at the specific heat values, we can see that gold (Au) has the smallest value of 0.129 J/g°C.
Therefore, the metal that will experience the largest temperature change when the same amount of heat is added is gold (Au). So, the correct answer is D - Au.