A pure carbon sample is used in a school laboratory practical. The sample has a mass of 6.00 g.
| Quantity | Value |
|---|---|
| Relative atomic mass of carbon, ArA_rAr | 12 |
| Avogadro constant | 6.02 × 1023 per mole |
For the calculations, use n=mAr\displaystyle n = \frac{m}{A_r}n=Arm, m=n×Arm = n \times A_rm=n×Ar and N=n×6.02×1023N = n \times 6.02 \times 10^{23}N=n×6.02×1023.
State the type of particle that the carbon sample is made of.
Calculate the amount of carbon in the sample, in moles.
Calculate how many carbon atoms are in the sample.
A separate portion of carbon has an amount of 0.250 mol. Calculate its mass.
142 exam-style questions on Edexcel GCSE Chemistry 2.6 Calculations involving masses, covering 2.6.1 Relative formula mass and percentage composition, 2.6.2 Empirical and molecular formulae, 2.6.3 Conservation of mass, 2.6.4 Reacting masses and concentration in g dm⁻³, 2.6.5 The mole and the Avogadro constant, and 2.6.6 Limiting reactants and stoichiometry. Each one has a worked solution and a mark scheme showing where the marks go.