A 10-kg piece of aluminum (which has a specific heat of 900 J/kg×°C) is warmed so that its temperature increases by 5.0 C°. How much heat was transferred into it?
Given the info provided, this is a simple Q=mc(delta)T question. Simply plug and chug.
m=10kg
c=specific heat = 900j/kgxC
(delta)T= 5 C
The answer should be 4.5x10^4 J
Oh, heating up aluminum, huh? Well, here's the scoop: the amount of heat transferred can be calculated using the formula Q = m × c × ΔT, where Q is the heat transferred, m is the mass, c is the specific heat, and ΔT is the change in temperature.
So, plugging in the numbers, we have Q = 10 kg × 900 J/kg×°C × 5.0 °C. Crunching the numbers, we get... *drumroll*... 45,000 J of heat transferred!
That's a lot of warmth for aluminum! I hope it enjoys its toasty temperature rise.
To calculate the amount of heat transferred into the aluminum, we can use the formula:
Q = m × c × ΔT
Where:
Q = heat transferred into the aluminum (Joules)
m = mass of the aluminum (kg)
c = specific heat of aluminum (J/kg×°C)
ΔT = change in temperature (°C)
Given:
m = 10 kg
c = 900 J/kg×°C
ΔT = 5.0 °C
Substituting the given values into the formula, we get:
Q = 10 kg × 900 J/kg×°C × 5.0 °C
Calculating this expression gives us:
Q = 45,000 Joules
Therefore, the amount of heat transferred into the aluminum is 45,000 Joules.
To calculate the amount of heat transferred to an object, you can use the formula:
Q = m * c * ΔT
where:
Q is the heat transferred
m is the mass of the object
c is the specific heat capacity of the material
ΔT is the change in temperature.
In this case, you are given:
m = 10 kg (mass of the aluminum)
c = 900 J/kg×°C (specific heat capacity of aluminum)
ΔT = 5.0 °C (change in temperature)
Plugging these values into the formula:
Q = 10 kg * 900 J/kg×°C * 5.0 °C
Now, multiply the numbers together:
Q = 45,000 J
Therefore, 45,000 Joules of heat were transferred into the aluminum.