In a calorimeter, there's 5mL of water. The temperature rises by 5 degrees (F).
How many calories are in the item put in the calorimeter?
To calculate the number of calories in the item put in the calorimeter, we need to use the equation Q = m * c * ΔT, where Q is the heat energy absorbed or released, m is the mass of the substance, c is the specific heat capacity of the substance, and ΔT is the change in temperature.
In this case, we have 5 mL (which is equivalent to 5 grams, assuming the density of water is 1 g/mL) of water and the temperature rises by 5 degrees Fahrenheit (ΔT = 5°F).
The specific heat capacity of water is approximately 1 calorie/gram °C (or approximately 4.18 joules/gram °C). Since we are working with Fahrenheit, we will need to convert the ΔT to Celsius.
To convert Fahrenheit to Celsius:
1. Subtract 32 from the Fahrenheit temperature.
2. Multiply the result by 5/9 to convert to Celsius.
Using these conversion steps, we can calculate ΔT in Celsius:
ΔT (°C) = (5°F - 32) * 5/9 = -15°C.
Now, we can calculate the heat energy absorbed or released (Q) by the water using the equation:
Q = m * c * ΔT = 5 g * 1 cal/g °C * (-15°C) = -75 calories.
Therefore, the item put in the calorimeter released 75 calories of heat energy.