d) Butane, C 4 H 10 , reacts with chlorine to give several products.(i) State the condition needed for this substitution reaction...................................................................................................................................... [1](ii) One of these products contains 37.8% carbon by mass, 6.30% hydrogen by mass and55.9% chlorine by mass.Calculate the empirical formula of the product.Deduce the molecular formula of the product.empirical formula ...............................................................molecular formula ...............................................................[3
Question
d) Butane, C 4 H 10 , reacts with chlorine to give several products.(i) State the condition needed for this substitution reaction...................................................................................................................................... 1 One of these products contains 37.8% carbon by mass, 6.30% hydrogen by mass and55.9% chlorine by mass.Calculate the empirical formula of the product.Deduce the molecular formula of the product.empirical formula ...............................................................molecular formula ...............................................................[3
Solution
(i) The condition needed for this substitution reaction is UV light or heat.
(ii) To calculate the empirical formula of the product, we first assume that we have 100g of the compound. This means that we have 37.8g of carbon, 6.30g of hydrogen, and 55.9g of chlorine.
Next, we convert these masses to moles. The molar mass of carbon (C) is approximately 12.01 g/mol, hydrogen (H) is approximately 1.01 g/mol, and chlorine (Cl) is approximately 35.45 g/mol.
So, we have:
- Carbon: 37.8g / 12.01 g/mol = 3.15 mol
- Hydrogen: 6.30g / 1.01 g/mol = 6.24 mol
- Chlorine: 55.9g / 35.45 g/mol = 1.58 mol
The empirical formula is the simplest, most reduced ratio of elements in a compound. To find this, we divide each of the calculated moles by the smallest number of moles calculated, which is 1.58:
- Carbon: 3.15 / 1.58 = 2
- Hydrogen: 6.24 / 1.58 = 4
- Chlorine: 1.58 / 1.58 = 1
So, the empirical formula is C2H4Cl.
To find the molecular formula, we need to know the molar mass of the compound. Butane reacts with chlorine to form a chloroalkane. The most likely product in this case would be butyl chloride, which has a molar mass of approximately 92.57 g/mol.
The empirical formula mass for C2H4Cl is (212.01) + (41.01) + 35.45 = 64.97 g/mol.
The ratio of the molecular mass to the empirical formula mass is 92.57 / 64.97 = 1.42, which is approximately 1 when rounded to the nearest whole number.
Therefore, the molecular formula is the same as the empirical formula, C2H4Cl.
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