What energy is required to heat water at #298*K# to water vapour at #373*K# under standard conditions?
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The energy required to heat water from 298 K to water vapor at 373 K under standard conditions can be calculated using the formula:
[ Q = mc\Delta T ]
Where:
- ( Q ) is the energy required (in joules).
- ( m ) is the mass of the water (in grams).
- ( c ) is the specific heat capacity of water (in J/g°C).
- ( \Delta T ) is the change in temperature (in °C).
Specific heat capacity of water is approximately (4.18 , \text{J/g°C}).
To find the energy required, we need to calculate the change in temperature (( \Delta T )) and then use it in the formula along with the mass of water.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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