The specific heat of copper is 0.385 J/g °C. How much thermal energy is required to increase the temperature of a 20g sample of copper from 20°C to 50°C?
231
20(0.385)(30) = 231
(0.385 J/g °C) * (50ºC - 20ºC) * 20g = ? Joules
Well, well, well, looks like we have ourselves a hot copper problem! So, let's calculate how much thermal energy we need.
First, we need to find the temperature difference between 50°C and 20°C. That's 30°C, my friend.
Now, multiply the mass of the copper (20g) by the specific heat (0.385 J/g °C) and the temperature difference (30°C). And voila! You'll end up with the amount of thermal energy required.
So, let me do the math for you: 20g * 0.385 J/g °C * 30°C = 231 J.
So, you'll need 231 Joules of thermal energy to heat up your copper sample. Hope that helps!
To calculate the amount of thermal energy required to increase the temperature of a substance, you can use the formula:
Q = m * c * ΔT
Where:
Q is the thermal energy (in joules),
m is the mass of the substance (in grams),
c is the specific heat capacity of the substance (in J/g °C),
ΔT is the change in temperature (in °C).
In this case, you want to find the amount of thermal energy required to increase the temperature of a 20g sample of copper from 20°C to 50°C. Therefore:
m = 20g (mass),
c = 0.385 J/g °C (specific heat capacity),
ΔT = 50°C - 20°C = 30°C (change in temperature).
Now, substitute these values into the formula and calculate the thermal energy (Q):
Q = 20g * 0.385 J/g °C * 30°C
Q = 231 J
Therefore, the amount of thermal energy required to increase the temperature of a 20g sample of copper from 20°C to 50°C is 231 Joules.