Please help me!!
350.0 ml of water is heated from 20.5 C to 98.2 C. What is the amount of energy required for this change?
In the decomposition of KCIO3 how many moles of KCI are formed in the reaction that produces 0.05 moles of O2?
q = mass H2O x specific heat H2O x (T final-T initial)
To calculate the amount of energy required for this change, you can use the formula:
Q = mcΔT
Where:
Q is the energy transferred (in joules)
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)
In this case, we are dealing with water. The specific heat capacity of water is approximately 4.18 J/g°C.
Step 1: Convert the volume of water to mass.
Since the density of water is 1 g/mL, the mass of water can be calculated using:
Mass = volume × density
= 350.0 mL × 1 g/mL
= 350.0 g
So, the mass of water is 350.0 grams.
Step 2: Calculate the change in temperature.
The change in temperature (ΔT) is given by the final temperature minus the initial temperature:
ΔT = Final temperature - Initial temperature
= 98.2°C - 20.5°C
= 77.7°C
Therefore, the change in temperature is 77.7°C.
Step 3: Calculate the energy required.
Now, plug the values into the formula:
Q = mcΔT
Q = (350.0 g) × (4.18 J/g°C) × (77.7°C)
Q ≈ 109,241.8 J
So, the amount of energy required for this change is approximately 109,241.8 joules.