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Step2247 [10]
1 year ago
13

in a fatty acid, the hydrogen atoms are of the double bond, which produces a kink in the carbon chain. in a fatty acid, the hydr

ogen atoms are of the double bond, which gives a carbon chain without any kink.
Chemistry
1 answer:
crimeas [40]1 year ago
4 0

In a CIS fatty acid, the hydrogen atoms are ON THE SAME SIDE of the double bond, which produces a kink in the carbon chain.

In a TRANS fatty acid, the hydrogen atoms are ON OPPOSITE SIDE of the double bond, which gives a carbon chain without any kink.

In unsaturated fatty acids (with one or more double bonds between carbon atoms), the cis double bonds cause the carbon chain to bend (kink), which gives the molecules an irregular shape (see the picture below).

Cis fatty acids are not as close as trans fatty acids, so they have fewer dispersion forces between their carbon chains.

Cis fatty acids have lower melting and boiling points than trans fatty acids.

More about cis and trans isomers: brainly.com/question/10407072

#SPJ4

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3 years ago
Determine the free energy(ΔG) from the standard cell potential (Ecell0 ) for the reaction:2ClO2-(aq)+Cl2(g)→2ClO2(g)+ 2Cl-(aq)wh
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<u>Answer:</u> The \Delta G^o for the given reaction is -7.84\times 10^4J

<u>Explanation:</u>

For the given chemical reaction:

2ClO_2^-(aq.)+Cl_2(g)\rightarrow 2ClO_2(g)+2Cl^-(aq.)

Half reactions for the given cell follows:

<u>Oxidation half reaction:</u> ClO_2^-\rightarrow ClO_2+e^-;E^o_{ClO_2^-/ClO_2}=0.954V  ( × 2)

<u>Reduction half reaction:</u> Cl_2+2e^-\rightarrow 2Cl(g);E^o_{Cl_2/2Cl^-}=1.36V

Oxidation reaction occurs at anode and reduction reaction occurs at cathode.

To calculate the E^o_{cell} of the reaction, we use the equation:

E^o_{cell}=E^o_{cathode}-E^o_{anode}

Putting values in above equation, we get:

E^o_{cell}=1.36-(0.954)=0.406V

To calculate standard Gibbs free energy, we use the equation:

\Delta G^o=-nFE^o_{cell}

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Putting values in above equation, we get:

\Delta G^o=-2\times 96500\times 0.406=-78358J=-7.84\times 10^4J

Hence, the \Delta G^o for the given reaction is -7.84\times 10^4J

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