Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations you made over the course of Part I.
Aluminum
Measured Mass of Metal 41.66 g Distilled Water Measurement 25 mL Distilled Water Temperature 25 C Temperature of Metals 100 C Temperature of Mixture 44.1 C
Part II:
Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations you made over the course of Part II.
Measured Mass of Metal 25.605 g Distilled Water Measurement 25 mL Distilled Water Temperature 25 C Temperature of Metals 100 C Temperature of Mixture 29.1 CCalculation’s:
Show your work and write a short explanation with each calculation.
Part I:
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
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.
Part II:
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. Show ALL your work.
The water has absorbed the heat of the metal. So, qwater = qunknown metal
2. Using the formula qunknown metal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the unknown metal in your calculation. Show ALL your work.
And how would you like for us to help you? The directions are there, the formulas are there, the only thing left is for you to substitute the numbers into the formula to obtain the answers.
We shall be happy to check your work.
yes
Part I:
Data Table:
Measured Mass of Metal: 41.66 g
Distilled Water Measurement: 25 mL
Distilled Water Temperature: 25°C
Temperature of Metals: 100°C
Temperature of Mixture: 44.1°C
Observations: No specific observations were mentioned in relation to Part I.
Calculations:
1. Calculate the energy change (q) of the surroundings (water) using the enthalpy equation:
q_water = m × c × ΔT
Given:
m = mass of water = 25 g
c = specific heat capacity of water = 4.18 J/(g × °C)
ΔT = change in temperature of water = (Temperature of Mixture - Distilled Water Temperature) = 44.1°C - 25°C = 19.1°C
Substitute the values into the equation:
q_water = 25 g × 4.18 J/(g × °C) × 19.1°C = 1,971.525 J
The energy change of the surroundings (water) is 1,971.525 J.
2. Using the formula q_metal = m × c × ΔT, calculate the specific heat of the metal:
Given:
q_metal = q_water = 1,971.525 J
m = mass of metal = 41.66 g
ΔT = change in temperature of metal = (Temperature of Metals - Temperature of Mixture) = 100°C - 44.1°C = 55.9°C
Rearranging the equation:
c = q_metal / (m × ΔT)
Substitute the values into the equation:
c = 1,971.525 J / (41.66 g × 55.9°C) = 0.872 J/(g × °C)
The specific heat of the metal is 0.872 J/(g × °C).
Part II:
Data Table:
Measured Mass of Metal: 25.605 g
Distilled Water Measurement: 25 mL
Distilled Water Temperature: 25°C
Temperature of Metals: 100°C
Temperature of Mixture: 29.1°C
Observations: No specific observations were mentioned in relation to Part II.
Calculations:
1. Calculate the energy change (q) of the surroundings (water) using the enthalpy equation:
q_water = m × c × ΔT
Given:
m = mass of water = 25 g
c = specific heat capacity of water = 4.18 J/(g × °C)
ΔT = change in temperature of water = (Temperature of Mixture - Distilled Water Temperature) = 29.1°C - 25°C = 4.1°C
Substitute the values into the equation:
q_water = 25 g × 4.18 J/(g × °C) × 4.1°C = 429.15 J
The energy change of the surroundings (water) is 429.15 J.
2. Using the formula q_unknown metal = m × c × ΔT, calculate the specific heat of the metal:
Given:
q_unknown metal = q_water = 429.15 J
m = mass of metal = 25.605 g
ΔT = change in temperature of metal = (Temperature of Metals - Temperature of Mixture) = 100°C - 29.1°C = 70.9°C
Rearranging the equation:
c = q_unknown metal / (m × ΔT)
Substitute the values into the equation:
c = 429.15 J / (25.605 g × 70.9°C) = 0.239 J/(g × °C)
The specific heat of the metal is 0.239 J/(g × °C).