Chemistry Stoichiometry SET 2019
PMDC Verified Question 74 of 105
A piece of diamond embedded in a gold ring weighs 6.0 gram. How many numbers of moles of Carbon does it contain?
A
6.0 mole
B
0.5 mole
C
1.0 mole
D
1.5 mole
Tap any option to test your recall and reveal the step-by-step Propolis autopsy.

Propolis Cognitive Error Autopsy

Official Correct Choice:
Option B: 0.5 mole
Concept:

Diamond is a purely carbon-based giant covalent structure. Therefore, the mass of a diamond is simply the mass of pure elemental Carbon.

Formula:

$$ n = \frac{m}{M} $$

Solution:

  • The chemical composition of a diamond is pure Carbon (C).


  • The molar mass of Carbon is \( 12 \text{ g/mol} \).


  • Given mass of the diamond = \( 6.0 \text{ g} \).


  • \( n = \frac{6.0 \text{ g}}{12 \text{ g/mol}} \).


  • \( n = 0.5 \text{ moles} \).


Why other options are incorrect:

  • 6.0 mole: Assumes the mass is directly equal to moles, ignoring molar mass.


  • 1.0 mole: Would require the diamond to weigh exactly 12 grams.


  • 1.5 mole: Would require the diamond to weigh exactly 18 grams.

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