Question 1 (1 point)
The heat of vaporization of methane, CH4, at its
boiling point is 9.20 kJ/mol. How much heat
energy is required to vaporize 100. g of methane
at its boiling point?

57.5 kj

Explanation:

Given data:

Heat of vaporization of  methane = 9.20 kj/mol

Heat energy required to vaporize 100 g of methane = ?

Solution:

First of all we will calculate the number of moles of methane in 100 g.

Number of moles of methane:

Number of moles = mass/ molar mass

Number  of moles = 100 g/ 16 g/mol

Number of moles = 6.25 mol

It is stated that for one mole of methane heat of vaporization is 9.20 kj.

For 6.25 mol or 100 g,

6.25 mol × 9.20 kj/mol

57.5 kj

specific gravity is the density of a substance divided by the density of water. since (at standard temperature and pressure) water has a density of 1 gram/cm3, and since all of the units cancel, specific gravity is usually very close to the same value as density

so "c" is the answer

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a pan containing water is placed in a positio n where it is exposed to a 10 mile per hour wind. the pan contains a uniform depth of 1.27 cm of water, is quite wide, and has a length of 2.44 m in the wind direction. the water in the pan is at a constant temperature of 15.5 °c.