Determine the amount of heat that must be added to raise the temperature of a cup of coffee ( 50.0 mL ) from 20.5ºC to 95.6ºC . Assume that water and coffee have the same density (1.00 g/mL) and same specific heat capacity ( 1 cal /g·°C).
q = heat needed = mass coffee x specific heat coffee x (Tfinal - Tinitial)
Substitute and solve for q. Tfinal is 95.6 from the problem. Tinitial is 20.5 from the problem. Post your work if you get stuck.
So it will be..
Q = (50.0mL) X (1cal) x ( 95.6 - 20.5) =
Is this the right set?
@DrBob222
To determine the amount of heat that must be added to raise the temperature of a cup of coffee, we can use the formula:
Q = mass x specific heat capacity x change in temperature
First, we need to determine the mass of the cup of coffee. We are given that the density of water and coffee is 1.00 g/mL, and the volume of the cup of coffee is 50.0 mL. Therefore, the mass can be calculated as:
mass = density x volume = 1.00 g/mL x 50.0 mL = 50.0 g
Next, we need to calculate the change in temperature. The initial temperature is 20.5ºC, and the final temperature is 95.6ºC. Therefore, the change in temperature can be calculated as:
change in temperature = final temperature - initial temperature = 95.6ºC - 20.5ºC = 75.1ºC
Now, we can substitute the values into the formula to find the amount of heat (Q):
Q = 50.0 g x 1 cal/g·°C x 75.1ºC = 3755 cal
Therefore, the amount of heat that must be added to raise the temperature of the cup of coffee from 20.5ºC to 95.6ºC is 3755 calories.