Question

A man ate 0.489 pound of cheese (an energy intake of 3.10 × 103 kJ). Suppose that none of the energy was stored in his body. What mass (in grams) of water would he need to perspire in order to maintain his original temperature? (It takes 44.0 kJ to vaporize 1 mole of water.) Enter your answer in scientific notation.

Answer 1

Answer: Mass of water required is 1268.18 g.

Step-by-step explanation:

It is mentioned that the energy intake of 0.489 pounds of cheese is 3100 kJ.

And, 1 mole of water takes 44.0 kJ of energy. Hence, we will calculate the molar mass of water as follows.

Molar mass of is =
`(2 * \text{Atomic mass of H}) + \text{Atomic mass of O}`

=
`(2 * 1) + 16`

= 18 g/mol

This means that 18 g of water takes 44.0 kJ of energy

. Therefore, mass of water required for 3100 kJ of energy will be calculated as follows.

Mass =
`((18 * 3100))/(44.0)`

= 1268.18 g of water

Thus, we can conclude that mass of water required is 1268.18 g.