Answer:
Compound A is CH3
Compound B is C6H.
Step-by-step explanation:
For compound A, the molar mass can be calculated by adding the atomic masses of carbon and hydrogen:
Molar mass of A = (6.3 g H / 1 g/mol H) + (18.7 g C / 12 g/mol C)
Molar mass of A = 0.525 mol H + 1.56 mol C
Molar mass of A = 2.085 g/mol
To find the empirical formula, we divide the number of moles of each element by the smallest number of moles:
H: 0.525 mol / 0.525 mol = 1
C: 1.56 mol / 0.525 mol = 2.97 ≈ 3
Therefore, the empirical formula for compound A is CH3.
For compound B, we follow the same steps:
Molar mass of B = (6.9 g H / 1 g/mol H) + (41.0 g C / 12 g/mol C)
Molar mass of B = 0.575 mol H + 3.42 mol C
Molar mass of B = 3.995 g/mol
Empirical formula:
H: 0.575 mol / 0.575 mol = 1
C: 3.42 mol / 0.575 mol = 5.95 ≈ 6
Therefore, the empirical formula for compound B is C6H.
To find the carbon to hydrogen mass ratio in each compound, we need to compare the ratios of their molar masses:
Carbon to hydrogen ratio in A = (1 * 12 g/mol) / (3 * 1 g/mol)
Carbon to hydrogen ratio in A = 4
Carbon to hydrogen ratio in B = (6 * 12 g/mol) / (1 * 1 g/mol)
Carbon to hydrogen ratio in B = 72
Therefore, the carbon to hydrogen mass ratio in compound A is 4:1 and in compound B is 72:1.