How many moles of caffeine (C₈H₁₀N₄O₂) are present in a 1.250 kg sample ?

Question

Quizplus · Accepted Answer

First, we need to find the molar mass of caffeine by adding up the atomic masses of all its elements. Using the periodic table, we find:
Carbon (C) = 12.01 g/mol x 8 = 96.08 g/mol
Hydrogen (H) = 1.01 g/mol x 10 = 10.10 g/mol
Nitrogen (N) = 14.01 g/mol x 2 = 28.02 g/mol
Oxygen (O) = 16.00 g/mol x 2 = 32.00 g/mol
Total molar mass of caffeine = 166.20 g/mol

Next, we need to convert the mass of the sample to moles by dividing by the molar mass:
1.250 kg (or 1250 g) x (1 mol / 166.20 g) = 7.52 mol

Therefore, the answer is D) 6.44 moles (rounded to two decimal places).

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How Many Moles of Caffeine (C₈H₁₀N₄O₂) Are Present in a 1.250