Question

The melting of ice at body temperature is an endothermic procesd thus eating ice counteracts exothermic metabolic reaction how much ice would you eat to counteract the heat produced by eating 28.3g of peanuts a)78g b) 1100grams?

Answer 1

I get c) 2210 g.

The heat produced depends on the type of peanuts and their "caloric value".

My nutrition table states that 100 g of raw, unsalted peanuts provide 2604 kJ.

So, from 28.3 g of peanuts,

`"Energy" = 28.3 color(red)(cancel(color(black)("g peanuts"))) × "2604 kJ"/(100 color(red)(cancel(color(black)("g peanuts")))) = "736.9 kJ"`

You must eat enough ice to absorb 736.9 kJ.

The formula for the quantity of heat `q` transferred is

`color(blue)(bar(ul(|color(white)(a/a)q = mΔ_text(fus)Hcolor(white)(a/a)|)))" "`

where

`m color(white)(mll) =` the mass of the ice
`Δ_text(fus)H` = the enthalpy of fusion of ice = 333.55 J/g

So,

`m = q/(Δ_text(fus)H)`

`m = ("736 900" color(red)(cancel(color(black)("J"))))/(333.55 color(red)(cancel(color(black)("J")))·"g"^"-1") = "2210 g"`

That's a lot of ice!