If 55.0 kJ of heat are added to 20.0 g of water at 20oC, what is the final temperature of the system?
q = mass x specific heat x (Tfinal-Tinitial)
Post your work if you get stuck.
So far i have
deltaH= 20g x 4.18 j/g deg C x 80 deg
= 6.688KJ
AND
DELTA H= 1.11mol x 40.8 KJ/Mol
= 45.3 kj
but i don't know what to do next :(
To determine the final temperature of the system, we can use the equation:
q = m * c * ΔT
Where:
q = heat added to the system (in joules)
m = mass of the substance (in grams)
c = specific heat capacity of the substance (in J/g·°C)
ΔT = change in temperature (in °C)
First, let's convert the given information to the correct units:
55.0 kJ = 55.0 * 1000 J (converting kilojoules to joules)
20.0 g (mass of water, already in grams)
The specific heat capacity of water is approximately 4.18 J/g·°C.
Next, we need to rearrange the equation to solve for ΔT:
ΔT = q / (m * c)
Substituting the known values:
ΔT = (55.0 * 1000 J) / (20.0 g * 4.18 J/g·°C)
Calculating:
ΔT ≈ 660.24 °C
Finally, to find the final temperature, we add the change in temperature to the initial temperature of 20°C:
Final temperature = 20°C + 660.24°C
The final temperature of the system is approximately 680.24°C.
To find the final temperature of the system, we need to use the equation:
q = m * c * ΔT
Where:
- q is the heat absorbed or released by the substance (in joules or in this case, kilojoules)
- m is the mass of the substance (in grams)
- c is the specific heat capacity of the substance (in J/g°C)
- ΔT is the change in temperature (in °C)
First, let's convert the kilojoules to joules since the specific heat capacity is usually given in J/g°C:
55.0 kJ = 55,000 J
The specific heat capacity of water is approximately 4.18 J/g°C. Now we can plug in the values:
q = m * c * ΔT
55,000 J = 20.0 g * 4.18 J/g°C * ΔT
We need to solve for ΔT, which represents the change in temperature. Rearranging the equation, we can isolate ΔT:
ΔT = q / (m * c)
Now we can substitute the values we know:
ΔT = 55,000 J / (20.0 g * 4.18 J/g°C)
Calculating this gives us:
ΔT = 55,000 J / (83.6 g°C) = 658.37 °C
Since we are starting at 20.0 °C, we need to determine the final temperature. Therefore, we add the ΔT to the initial temperature:
Final temperature = Initial temperature + ΔT
Final temperature = 20.0 °C + 658.37 °C = 678.37 °C
So, the final temperature of the system is approximately 678.37 °C.