Calculate the amount of heat required to heat a 3.5 kg gold bar from 21 degrees C to 37 degrees C. What would be the best way to work this problem? I don't know if I need to convert the kg to g.
First you must have the specific heat of gold. That may be in your problem or in tables in the back of your text. If not you can look it up on Google. Use it in joules/g*oC. Then
q = mass x specific heat x (Tfinal-Tinitial)
If specific heat is in grams*degreesC then convert kg to grams.
To calculate the amount of heat required, you will need to use the equation Q = mcΔT, where Q is the heat energy, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
1. First, let's calculate the mass of the gold bar (m). No conversion is needed since the mass is already given in kilograms as 3.5 kg.
2. Next, find the specific heat capacity (c) of gold. The specific heat capacity of gold is approximately 129 J/(kg·°C).
3. Calculate the change in temperature (ΔT) by subtracting the initial temperature (21°C) from the final temperature (37°C). ΔT = 37°C - 21°C = 16°C.
4. Finally, substitute the values into the equation Q = mcΔT.
Q = (3.5 kg) * (129 J/(kg·°C)) * (16°C)
Q = 7104 J
Therefore, the amount of heat required to heat the 3.5 kg gold bar from 21°C to 37°C is 7104 Joules. No conversion to grams is needed for this calculation.