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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
 one year ago
 one year 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
 one year ago
 one year ago

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AshjaBest ResponseYou've already chosen the best response.1
2. 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.
 one year ago

goformit100Best ResponseYou've already chosen the best response.0
put their values in it
 one year ago
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