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Compare the specific heat capacities

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Reference no: EM132762186

Note and record the specific heat capacity of silver, gold, copper, and iron by selecting each metal and reading the respective "Specific Heat" value; convert to J/(kg·°C) by multiplying by 1000. Run the simulation to answer the following questions. Your quantitative analysis may be performed by writing out the correct formula, substituting the numbers observed from the simulation, and expressing the answer correctly in terms of units and significant digits.

1. If you kept the mass and starting temperature of each metal and the mass and starting temperature of the water constant, which sample of hot metal would generate the greatest temperature change in the water? Verify your guess

2. Let's compare the specific heat capacities of 20 g samples of gold and iron. Set the following for each scenario:

The starting mass and temperature for water, in each of the two scenarios, are 30 g and 20 °C, respectively. Set the initial metal temperature to 200 °C. Perform the two simulations and record their respective final temperatures to find out which transferred more heat to the water.

3. Place a cold piece of any of the first four metals into some water that is hotter than the metal. Perform the simulation, record the final temperature, and analyze the results to compare the heat absorbed by the metal and the heat lost by the water.

4. Run the simulation to find the specific heat capacities of metal X and Y. Research the specific heats of metals and try to identify each mystery metal.

5. Place a 50 g cube of ice into 200 g of 40 °C water. Perform the simulation, record the final temperature, and analyze the results to find out if the thermal energy lost by the water equals the thermal energy gained by the ice. Assuming the thermal energy lost by the water is correct, find the percentage error in the simulation. The latent heat of fusion of ice is 3.3 x 105 J/kg.

In addition carefully sketch the temperature versus time graph (the cooling curve). Add a line to show the ice changing state and then warming up within the calorimeter. Label the cooling curve to explain what is taking place in both lines at the beginning, middle, and end.

Reference no: EM132762186

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