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In compound A, there is 6.3 g of hydrogen and 18.7 g of carbon, while in compound B there is 6.9 g of hydrogen and 41.0 g of carbon, what is the carbon to hydrogen mass ratio in each compound and how do these ratios compare?

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1 vote

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.

User DKab
by
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2 votes

Answer: No, compound A and B are not the same compound

Explanation:easy

User Tomasz Kula
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8.2k points

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