Question

What if the pot were made of aluminum? Calculate the heat required for an aluminum pot to heat up by 75.0C. The mass of the pot is now 1.74kg, since aluminum is much less dense than iron.

Q= m * c * △t = _____ *_____ *_____ = _____ joules

Answer 1

Q = 1,740 * 0.903 * 75.0= 117,202.5 Joules

Step-by-step explanation:

Just like before, the equation Q = m * c * Δt can be used to calculate the amount of heat energy required to heat up the aluminum pot.

In this case, we have:

m = 1.74 kg (the mass of the aluminum pot)

c = 0.903 J/g°C (the specific heat of aluminum)

Δt = 75.0°C (the change in temperature needed to heat up the aluminum pot)

We need to convert the mass of the pot from kilograms to grams, since the specific heat is given in Joules per gram per degree Celsius:

m = 1,740 grams

Now we can plug in these values and solve for Q:

Q = m * c * Δt

Q = 1,740 * 0.903 * 75.0

Q = 117,202.5 Joules

So it would take 117,202.5 Joules of heat energy to heat up the aluminum pot by 75.0°C.