Chlorination of methane takes place by:
1. Elimination
2.
3. Free radical
4.
The products formed after ozonolysis of Pent-2-ene are:
1. Ethanal and Methanal
2. Ethanal and Propanal
3. Ethanal and Butanal
4. Ethanal and Ethanal
Decreasing order of acidic behavior of benzene, n-hexane, and ethyne is -
1. Hexane > Ethyne > Benzene
2. Benzene > Hexane > Ethyne
3. Ethyne > Benzene > Hexane
4. Benzene > Ethyne > Hexene
Out of the above alkenes, the ones that can give 2-methyl butane on hydrogenation are-
1. | a, b | 2. | b, c |
3. | a, c | 4. | a, b, c |
The correct order of decreasing reactivity of the following compounds:
Chlorobenzene, 2,4-Dinitrochlorobenzene, and p-Nitrochlorobenzene
with an electrophile (E+) is :
1. | Chlorobenzene > p–Nitrochlorobenzene > 2,4-Dinitrochlorobenzene |
2. | p – Nitro chlorobenzene > 2, 4-Dinitrochlorobenzene > Chlorobenzene |
3. | Chlorobenzene > 2, 4-Dinitrochlorobenzene > p-Nitrochlorobenzene |
4. | 2, 4-Dinitrochlorobenzene > Chlorobenzene > p-Nitrochlorobenzene |
An alkene ‘A’ on ozonolysis gives a mixture of ethanal and pentan-3-one.
The IUPAC name of ‘A’ is :
1. 3-Ethylpent-2-ene
2. 3-Ethylpent-2- yne
3. 2-Ethylpent-3-ene
4. 3-Ethylpent-4-yne
An alkene ‘A’ contains 3 C – Cσ bonds, 8 C – H σ bonds, and 1 C – C π bond,
‘A’ on ozonolysis gives two moles of an aldehyde of molar mass 44 u. The IUPAC name of ‘A’ is -
1. Prop-2-yne
2. But-2-ene
3. But-2-yne
4. Prop-2-ene
Propanal and pentane-3-one are the products of ozonolysis of an alkene. The structural formula of the alkene is :
1. | 2. | , | |
3. | 4. |
The balanced chemical equation for the combustion reaction of Butane is :
1. | \(2 \mathrm{C}_4 \mathrm{H}_{10(\mathrm{~g})}+13 \mathrm{O}_{2(\mathrm{~g})} \rightarrow 8 \mathrm{CO}_{2(\mathrm{~g})}+10 \mathrm{H}_2 \mathrm{O}+\text { Heat }\) Butane |
2. | \(2 \mathrm{C}_4 \mathrm{H}_{10(\mathrm{~g})}+13 \mathrm{O}_{2(\mathrm{~g})} \rightarrow 9 \mathrm{CO}_{2(\mathrm{~g})}+10 \mathrm{H}_2 \mathrm{O}+\text { Heat }\) Butane |
3. | \(2 \mathrm{C}_4 \mathrm{H}_{10(\mathrm{g})}+14 \mathrm{O}_{2(\mathrm{g})} \rightarrow 8 \mathrm{CO}_{(\mathrm{g})}+10 \mathrm{H}_2 \mathrm{O}+\text { Heat }\) Butane |
4. | \( \mathrm{C}_4 \mathrm{H}_{10(\mathrm{~g})}+13 \mathrm{O}_{2(\mathrm{g})} \rightarrow 8 \mathrm{CO}_{(\mathrm{g})}+10 \mathrm{H}_2 \mathrm{O}+\text { Heat }\) Butane |