Assume the heat absorbed by the calorimeter was 200J. What is the calorimeter constant (Heat Capacity) if the temperature changed from 22C to 26C?

I know the answer is 50 J/k. But I am not sure how to get this.

q = Qcal x delta T

200 = Qcal x 4

Thank you!

Well, well, well, looks like we've got a hot question here! Let's break it down and spice it up with a little humor, shall we?

To find the calorimeter constant, or heat capacity, we need to use the formula:

Heat Absorbed = Calorimeter Constant x Temperature Change

In our tasty scenario, we know the heat absorbed is 200 J, and the temperature changed from 22°C to 26°C. So, plugging in these values, we get:

200 J = Calorimeter Constant x (26°C - 22°C)

Now, let's do some math magic:

200 J = Calorimeter Constant x 4°C

To find the Calorimeter Constant, we simply divide both sides by 4°C:

Calorimeter Constant = 200 J / 4°C

And voila! The Calorimeter Constant is 50 J/°C (or J/K, as they have the same units). Isn't that "heatingly" cool?

So remember, when it comes to finding the Calorimeter Constant, just divide the heat absorbed by the temperature change, and you'll be cooking with gas! Keep up the great work, hotshot!

To find the calorimeter constant (heat capacity) of the calorimeter, we need to use the equation:

Q = CΔT

Where:
Q = heat absorbed by the calorimeter
C = calorimeter constant (heat capacity)
ΔT = change in temperature

Given:
Q = 200 J
ΔT = 26°C - 22°C = 4°C

Plugging in these values into the equation, we have:

200 J = C * 4°C

To isolate C, divide both sides of the equation by 4°C:

C = 200 J / 4°C

Simplifying the equation, we get:

C = 50 J/°C

Therefore, the calorimeter constant (heat capacity) is 50 J/°C or 50 J/K (since the units for temperature change are the same in J/°C and J/K).

To calculate the calorimeter constant (heat capacity), you need to use the equation:

Q = C * ΔT

where Q is the heat absorbed by the calorimeter, C is the calorimeter constant, and ΔT is the change in temperature.

In this case, you are given that the heat absorbed by the calorimeter is 200J and the temperature change is from 22°C to 26°C.

First, calculate the change in temperature (ΔT):

ΔT = Final Temperature - Initial Temperature
= 26°C - 22°C
= 4°C

Now, substitute the values into the equation and solve for C:

200J = C * 4°C

Divide both sides of the equation by 4°C:

200J / 4°C = C

C = 50 J/°C

So, the calorimeter constant (heat capacity) is 50 J/°C or 50 J/K (since the change in temperature is the same in both Celsius and Kelvin scales).

Note that the calorimeter constant represents the amount of heat energy required to raise the temperature of the calorimeter by 1 degree Celsius (or Kelvin).