A 47kg sample of water absorbs 3.40×10^2kJ of heat.
Part A
If the water was initially at 21.5∘C, what is its final temperature?
To find the final temperature of the water, we can use the formula:
q = mcΔT
Where:
- q is the heat absorbed by the water (3.40×10^2 kJ)
- m is the mass of the water (47 kg)
- c is the specific heat capacity of water (4.18 kJ/kg∙°C)
- ΔT is the change in temperature (Tf - Ti)
We want to find the final temperature Tf, so we rearrange the formula:
ΔT = q / (mc)
Now we can plug in the known values:
ΔT = (3.40×10^2 kJ) / (47 kg * 4.18 kJ/kg∙°C)
Calculating this will give us the change in temperature. To find the final temperature, we need to add this change to the initial temperature:
Tf = Ti + ΔT
Given that the initial temperature Ti is 21.5°C, we can add the change to it to get the final temperature.
Easy!
Using Q = mc(delta)
where delta = difference between final and initial temperature
Given m = 47 kg
Q = 3.40 X 10^2 kJ
Since heat is being absorbed into the system, this is an endothermic reaction.
c for water is 4.2 kJ/kg.C
Substituting Q,m,c & initial temperature of water into the equation.....
The final temperature is 23.2 degree C