To vaporize 35g of liquid water, multiply the mass of water (35g) by the heat of vaporization (2,250 J/g). The energy required is 78,750 J, so the closest answer choice is D) 79,100 J, assuming some rounding for the heat of vaporization value.
To determine how much energy is needed to vaporize 35g of liquid water, we use the heat of vaporization of water, which is about 2,250 J per gram. The equation to calculate the energy required for vaporization is Q = mLv, where Q is the energy in joules, m is the mass in grams, and Lv is the latent heat of vaporization in joules per gram.
By plugging in the values, we get:
Q = (35 g)(2,250 J/g) = 78,750 J
The closest answer choice to our calculation is D) 79,100 J, which likely accounts for the rounding of the heat of vaporization's exact value.