Calculate the amount of energy needed to vapourise 1.5 kg of water in the kettle. Use the equation Q = mL. The specific latent heat of vapourisation of water is 2.26 x 10^6 J kg^-1... Calculate the amount of energy needed to vapourise 1.5 kg of water in the kettle. Use the equation Q = mL. The specific latent heat of vapourisation of water is 2.26 x 10^6 J kg^-1. Show your working.
Understand the Problem
The question is asking for the calculation of energy required to vaporize 1.5 kg of water using the provided specific latent heat of vaporization. It involves applying the equation Q = mL, where Q is the energy, m is the mass of the water, and L is the specific latent heat.
Answer
$Q = 3.39 \times 10^6 \, \text{J}$
Answer for screen readers
The amount of energy needed to vaporize 1.5 kg of water is $Q = 3.39 \times 10^6 , \text{J}$.
Steps to Solve
- Identify the variables in the equation
In the equation $Q = mL$, we identify the variables:
- $m$: mass of water = 1.5 kg
- $L$: specific latent heat of vaporization = $2.26 \times 10^6 , \text{J kg}^{-1}$
- Substitute the values into the equation
We substitute the values of $m$ and $L$ into the equation: $$ Q = 1.5 , \text{kg} \times 2.26 \times 10^6 , \text{J kg}^{-1} $$
- Perform the multiplication
Next, we perform the multiplication to calculate $Q$: $$ Q = 1.5 \times 2.26 \times 10^6 = 3.39 \times 10^6 , \text{J} $$
The amount of energy needed to vaporize 1.5 kg of water is $Q = 3.39 \times 10^6 , \text{J}$.
More Information
This result indicates the total energy needed to convert 1.5 kg of water at 100°C to vapor without changing temperature. It highlights the energy-intensive nature of the phase change from liquid to gas.
Tips
- Incorrect mass or latent heat value: Ensure that the mass and specific latent heat values are accurately taken from the problem.
- Miscalculating the multiplication: Double-check arithmetic steps when multiplying values in scientific notation.
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