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anonymous
 3 years ago
Metal: Aluminum
Mass of metal: 27.776 g
Volume of water in the calorimeter: 26.0 mL
Initial temperature of water in calorimeter: 25.3 °C
Temperature of hot water and metal in hot water bath: 100.5 °C
Final temperature reached in the calorimeter: 31.6 °C
1. Calculate the energy change (q) of the surroundings (water) using the enthalpy equation
qwater = m × c × ΔT.
We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL.
The water has absorbed the heat of the metal. So, qwater = qmetal
anonymous
 3 years ago
Metal: Aluminum Mass of metal: 27.776 g Volume of water in the calorimeter: 26.0 mL Initial temperature of water in calorimeter: 25.3 °C Temperature of hot water and metal in hot water bath: 100.5 °C Final temperature reached in the calorimeter: 31.6 °C 1. Calculate the energy change (q) of the surroundings (water) using the enthalpy equation qwater = m × c × ΔT. We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL. The water has absorbed the heat of the metal. So, qwater = qmetal

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anonymous
 3 years ago
Best ResponseYou've already chosen the best response.02. Using the formula qmetal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the metal in your calculation.

goformit100
 3 years ago
Best ResponseYou've already chosen the best response.0put their values in it
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