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
To calculate the energy change of the surroundings (water), we can use the enthalpy equation:
qwater = m × c × ΔT
where:
- qwater represents the energy change of water
- m represents the mass of water
- c represents the specific heat capacity of water
- ΔT represents the change in temperature
Given that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL, we can assume that the mass of water is equal to the volume of water.
First, we need to determine the mass of water. Since 1 mL of water weighs 1 g, the mass of water is equal to the volume of water. Therefore, the mass of water is equal to the mass of the unknown metal.
Now, let's say the mass of the metal is "m" grams.
Next, we need to determine the change in temperature (ΔT) of the water. This can be found by subtracting the initial temperature of the water from the final temperature of the water.
Let's say the initial temperature of the water is "T1" °C, and the final temperature of the water after absorbing the heat from the metal is "T2" °C. So, the change in temperature (ΔT) is equal to T2 minus T1.
Putting it all together, the equation becomes:
qwater = m × c × ΔT
Now, substitute the values you know into the equation and solve for qwater.
Make sure to use consistent units throughout the calculation.