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How much energy is needed to vaporize 5.00 g of water?

Answer 1

Wyatt Adkins

We need the enthalpy of vaporization of water.......

Regarding the response.

#H_2O(l) +Delta rarr H_2O(g)#

WHERE BOTH PRODUCT AND REACTANT ARE AT #100# #""^@C#, ..........

#DeltaH_"vaporization"^@=40.66*kJ*mol^-1#

Therefore, we must determine the molar amount of water that has evaporated.

#DeltaH_"rxn"=(5.00*g)/(18.01*g*mol^-1)xx40.66*kJ*mol^-1=11.3*kJ#.

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Answer 2

Caleb Adams

The amount of energy needed to vaporize a substance can be calculated using the formula:

Energy = mass × heat of vaporization

For water, the heat of vaporization is approximately 40.79 kJ/mol.

First, convert the mass of water from grams to moles using its molar mass (18.015 g/mol), then multiply by the heat of vaporization to get the energy required.

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Answer from HIX Tutor

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.