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 capacities of the metals. The specific heat capacity is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius.
From the chart, we can see that the metals are given in alphabetical order. Therefore, let's look up the specific heat capacities of each metal:
A (Ca) - Specific heat capacity = 0.647 J/g°C
B (Fe) - Specific heat capacity = 0.449 J/g°C
C (Ag) - Specific heat capacity = 0.235 J/g°C
D (Au) - Specific heat capacity = 0.128 J/g°C
Now, we need to calculate the temperature change for each metal. We'll assume that the same amount of heat is added to each sample (25.0 g):
A (Ca): Temperature change = Heat added / (Specific heat capacity x Mass) = Heat added / (0.647 J/g°C x 25.0 g)
B (Fe): Temperature change = Heat added / (0.449 J/g°C x 25.0 g)
C (Ag): Temperature change = Heat added / (0.235 J/g°C x 25.0 g)
D (Au): Temperature change = Heat added / (0.128 J/g°C x 25.0 g)
Since the same amount of heat is added to each metal, the denominator of each calculation is the same. Therefore, we just need to compare the numerators (the Heat added) to determine which metal will experience the largest temperature change.
Assuming the heat added is the same for each metal, we can conclude that the metal with the largest temperature change will be the one with the smallest specific heat capacity.
Therefore, from the given options, the metal that will experience the largest temperature change is:
D. Au (Gold), with a specific heat capacity of 0.128 J/g°C.
To determine which metal will experience the largest temperature change when the same amount of heat is added, we need to calculate the specific heat capacity for each metal and then compare them.
The specific heat capacity (c) is the amount of heat energy required to raise the temperature of a substance by 1 degree Celsius per unit mass. The equation for calculating heat (q) is q = mcΔT, where m is the mass, c is the specific heat capacity, and ΔT is the temperature change.
First, we need to find the specific heat capacity for each metal. The specific heat capacity values for the metals can be found in a reference source or table. Let's assume the values are:
A (Ca): 0.647 J/g°C
B (Fe): 0.449 J/g°C
C (Ag): 0.235 J/g°C
D (Au): 0.129 J/g°C
Next, we calculate the amount of heat for each metal using the equation q = mcΔT. We assume the same amount of heat is added to each metal sample, so the value of q will be the same for all metals.
Let's work through an example assuming a temperature change of 10°C:
For metal A (Ca), q = (25.0 g)(0.647 J/g°C)(10°C) = 161.75 J
For metal B (Fe), q = (25.0 g)(0.449 J/g°C)(10°C) = 112.25 J
For metal C (Ag), q = (25.0 g)(0.235 J/g°C)(10°C) = 58.75 J
For metal D (Au), q = (25.0 g)(0.129 J/g°C)(10°C) = 32.25 J
From the calculations, we can see that metal A (Ca) will experience the largest temperature change, as it requires the most heat energy to raise its temperature by the same amount compared to the other metals.
Therefore, the answer is A (Ca) – Calcium.