Order the relative rate of diffusion of the following gases from slowest to fastest. Kr, N, Ar, Ne.
2 answers:
Answer:
The increasing order relative rate of diffusion from fastest to slowest will be: N>Ne>Ar>Kr
Explanation:
Graham's diffusion law states that the rate of diffusion of gas is inversely proportional to the square root of the molecular mass of the gas. Mathematically given as:
Higher the molecular mass slower will be the diffusion rate.In the given gases the molecular mass of Krypton, nitrogen ,argon and neon is 83.80 g/mol,14.01 g/mol,39.95 g/mol and 20.18 g/mol respectively.
Increasing order of molecular mass: Kr >Ar>Ne> N
So, increasing order relative rate of diffusion from fastest to slowest will be: N>Ne>Ar>Kr
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Answer:
See explanation below
Explanation:
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For question 6a, as it was stated before, the mechanism in that reaction is a Sn2, however, we can have conditions for an E2 reaction and form an alkene. This can be done, cause the extoxide can substract the atoms of hydrogens from either the carbon of the cycle or the terminal methyl of the molecule and will form two different products of elimination. The product formed in greater quantities will be the one where the negative charge is more stable, in this case, in the primary carbon of the methyl it's more stable there, so product 1 will be formed more (See picture 2)
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