We apply the same amount of energy to 10.0-g samples of aluminum, and silver which begin at the same
temperature.Rank the metals from highest to lowest temperature after the heat is applied.
q = mass x specific heat x (Tfinal-Tinitial)
q = same. mass is same, Ti = same. sp. h. is not the same so Tfinal must change to account for that. One will have a higher final T than the other one.
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To rank the metals from highest to lowest temperature after applying the same amount of energy, we need to consider their specific heat capacities.
Specific heat capacity (c) is the amount of heat energy required to raise the temperature of a substance by 1 degree Celsius. The formula for heat energy is Q = mcΔT, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
Given that the same amount of energy is applied to 10.0-g samples of aluminum and silver starting at the same temperature, the masses (m) can be considered equal.
Comparing the specific heat capacities of aluminum and silver, we find that aluminum has a specific heat capacity of 0.903 J/g°C and silver has a specific heat capacity of 0.235 J/g°C.
Since aluminum has a higher specific heat capacity, it can absorb a larger amount of heat energy for the same increase in temperature compared to silver. Therefore, aluminum will reach a higher temperature than silver when the same amount of energy is applied.
Ranking the metals from highest to lowest temperature after applying the same amount of energy:
1. Aluminum
2. Silver
To rank the metals from highest to lowest temperature after applying the same amount of energy, we need to consider the specific heat capacity and mass of each metal.
The specific heat capacity (C) of a substance represents the amount of energy required to raise the temperature of a given mass of the substance by 1 degree Celsius.
Steps to calculate the temperature increase for each metal:
1. Determine the specific heat capacity of aluminum (C_al) and silver (C_ag). The specific heat capacity values can be found in reference materials or online databases. For example, the specific heat capacity of aluminum is approximately 0.897 J/g°C, and the specific heat capacity of silver is around 0.235 J/g°C.
2. Calculate the energy (Q) required to increase the temperature of each metal sample using the formula:
Q = mass * specific heat capacity * temperature change
Since the energy applied is the same for both metals, we can set Q_al = Q_ag.
3. Rearrange the formula to solve for the temperature change (ΔT):
ΔT = Q / (mass * specific heat capacity)
4. Calculate the temperature change for aluminum (ΔT_al) and silver (ΔT_ag) separately.
5. Add the initial temperature to the temperature change to find the final temperatures for each metal.
6. Rank the metals in order of highest to lowest final temperature.
Note: In this scenario, we assume that there are no heat losses to the surroundings and that the specific heat capacities are constant within the temperature range being considered.
By following these steps, you can calculate the final temperatures for aluminum and silver and rank them accordingly.