An average cup of coffee contains about 125 mg of caffeine, $C_8H_10N_4O_2$ . How many moles of caffeine are in a cup, and how many molecules of caffeine?

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Answer 1 · 2015-11-22T20:58:57

Enough caffeine to keep you up at night?

The molecular mass of caffeine is $194.19$ $g*mol^-1$ .

Moles of caffeine in a cup $=$ $(125xx10^-3g)/(194.19*g*mol^-1$ $=$ $??$ $mol$ .

The above calculation gives an answer in moles. This is simply a number, i.e. $N_A*mol*xx(125xx10^-3g)/(194.19*g*mol^-1$ $=$ $??$

An average cup of coffee contains about 125 mg of caffeine, C_8H_10N_4O_2C_8H_10N_4O_2. How many moles of caffeine are in a cup, and how many molecules of caffeine?