A 2.70g vitamin C tablet is found to contain 0.0109 mol of ascorbic acid (C6H806}. The molar mass of C6H806 is 176.12 g/mol. What
is the mass percent of C6H806 in the tablet?

We are given:

Mass of the tablet  = 2.7 grams

Number of moles of Ascorbic acid present in the tablet = 0.0109 moles

Molar mass of Ascorbic acid = 176.12 g/mol

Mass of Ascorbic Acid present in the tablet:

Mass of a given number of moles  = number of moles * molar mass

replacing the variables

Mass = 0.0109 * 176.12

Mass = 1.92 grams (approx)

Mass percent of Ascorbic acid:

Mass% = () * 100

replacing the variables

Mass% = (1.92 / 2.7) * 100

Mass% = 192 / 2.7

Mass% = 71.12 %

Therefore, the tablet has 71.12% Ascorbic Acid by mass

is it a purebred? it looks more like a red nose, but it doesn't have the red could it be a staffordshire bull terrior? unsure if that's the right name for it sorry

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explanation: