How joules many are needed to heat 1500 gram pot of water up to (100c) water temp is 22c
You need to learn and use this formula>:
Q = M*C*(delta T)
Q is the heat required
M is the mass,
C is the specific heat (4.18 J/g*degC), and delta T is the temperature change
Q = 1500*(4.18)*78 = _____ J
To find out how many joules are needed to heat a 1500 gram pot of water from 22°C to 100°C, we can use the formula:
Q = m * c * ΔT
Where:
Q is the amount of heat energy absorbed or released (in joules),
m is the mass of the substance (in grams),
c is the specific heat capacity of the substance (in joules per gram per degree Celsius),
ΔT is the change in temperature (in degrees Celsius).
In this case, the specific heat capacity of water is approximately 4.18 joules per gram per degree Celsius.
First, we need to calculate the change in temperature:
ΔT = 100°C - 22°C = 78°C
Now we can substitute the values into the formula:
Q = 1500g * 4.18 J/g°C * 78°C
Q ≈ 475,140 joules
Therefore, approximately 475,140 joules of energy are needed to heat a 1500 gram pot of water from 22°C to 100°C.