How many joules of heat are required to raise the temperature of 225 g of water from 42 degree celcius to 75 degree celcius?
q = mass H2O x specific heat H2O x (Tfinal-Tinitial)
Formula q=m*c*delT
data
m= 225gm
c= 1
delT= 75-42=33degree celcius
q=mct
=225*1.0*33
=7425 j
To calculate the amount of heat energy required, you need to use the formula:
Q = m * c * ΔT
Where:
Q = heat energy (in joules)
m = mass of water (in grams)
c = specific heat capacity of water (4.184 J/g°C)
ΔT = change in temperature (final temperature - initial temperature)
Given:
m = 225 g
c = 4.184 J/g°C
ΔT = (75°C - 42°C) = 33°C
Now, substitute the given values into the formula:
Q = 225 g * 4.184 J/g°C * 33°C
Q = 301,427.4 J
Therefore, approximately 301,427.4 joules (J) of heat are required to raise the temperature of 225 g of water from 42°C to 75°C.
To calculate the amount of heat required to raise the temperature of a substance, you can use the equation:
Q = mcΔT
Where:
Q is the heat energy in joules (J)
m is the mass of the substance in grams (g)
c is the specific heat capacity of the substance (in this case, water) in joules per gram degree Celsius (J/g°C)
ΔT is the change in temperature in degrees Celsius (°C)
First, let's find the specific heat capacity of water. The specific heat capacity of water is approximately 4.18 J/g°C.
Now, we can plug the given values into the equation:
m = 225 g (mass of water)
ΔT = (75°C - 42°C) = 33°C (change in temperature)
c = 4.18 J/g°C (specific heat capacity of water)
Q = (225 g) * (4.18 J/g°C) * (33°C)
Q = 31522.5 J
Therefore, approximately 31522.5 joules of heat are required to raise the temperature of 225 g of water from 42°C to 75°C.