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sukhopar [10]
4 years ago
14

There are four compounds with the

Chemistry
1 answer:
Oliga [24]4 years ago
4 0

Answer:

The four compounds with formula C4H9Br are

1. 1- Bromobutane

2. 2-Bromobutane

3. 1-bromo-2-methyl propane

4. 2-Bromo-2-methyl propane

Reactivity towards SN2 in decreasing order is :

1- Bromobutane >  1-bromo-2-methyl propane > 2-Bromobutane >

2-Bromo-2-methyl propane

Explanation:

SN2 reaction : This is also known as second order nucleophilic Substitution Reaction because :

  • The rate determining step depends both on the concentration of the substrate as well as nucleophile.
  • This reaction involve formation of 5- bond transition state (not the intermediate)
  • The bond making and breaking occur simultaneously
  • The reactivitey order for SN2 is more for less hindered substrate i.e :

Primary > Secondary > tertiary

Among the isomers of C4H9Br

  • <u>The primary halides are : 1- Bromobutane and 1-bromo-2-methyl propane</u>

(Br is attached to primary carbon)

but 1- Bromobutane is less hindered than 1-bromo-2-methyl propane

So,1- Bromobutane >  1-bromo-2-methyl propane

  • <u>Secondary :2-Bromobutane</u>
  • <u>Tertiary : 2-Bromo-2-methyl propane</u>

Hence order is :

1- Bromobutane >  1-bromo-2-methyl propane > 2-Bromobutane >

2-Bromo-2-methyl propane

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0.36 M

Explanation:

There is some info missing. I think this is the complete question.

<em>Suppose a 250 mL flask is filled with 0.30 mol of N₂ and 0.70 mol of NO. The following reaction becomes possible: </em>

<em>N₂(g) +O₂(g) ⇄ 2 NO(g) </em>

<em>The equilibrium constant K for this reaction is 7.70 at the temperature of the flask.  Calculate the equilibrium molarity of O₂. Round your answer to two decimal places.</em>

<em />

Initially, there is no O₂, so the reaction can only proceed to the left to attain equilibrium. The initial concentrations of the other substances are:

[N₂] = 0.30 mol / 0.250 L = 1.2 M

[NO] = 0.70 mol / 0.250 L = 2.8 M

We can find the concentrations at equilibrium using an ICE Chart. We recognize 3 stages (Initial, Change, and Equilibrium) and complete each row with the concentration or change in the concentration.

    N₂(g) +O₂(g) ⇄ 2 NO(g)

I    1.2        0              2.8

C  +x         +x            -2x

E  1.2+x      x           2.8 - 2x

The equilibrium constant (K) is:

K=7.70=\frac{[NO]^{2}}{[N_{2}][O_{2}]} =\frac{(2.8-2x)^{2} }{(1.2+x).x}

Solving for x, the positive one is x = 0.3601 M

[O₂] = 0.3601 M ≈ 0.36 M

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Suppose the formation of nitrosyl chloride proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) +
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Answer:

Overall reaction equation;

2NO(g) +Cl2(g) -----> 2NOCl (g)

Explanation:

Given

1) NO(g) + Cl2(g) → NOCl2(g)

2) NOCl2(g) + NO(g) → 2NOCl(g)

Overall reaction equation;

2NO(g) +Cl2(g) -----> 2NOCl (g)

k1= [NOCl2]

k-1= [NO] [Cl2]

k2 = [NOCl2] [NO]

Equilibrium for the first equation (reaction 1)

K= k1/k-1 = [NOCl2]/[NO] [Cl2]

Therefore

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Where Koverall= k1k2/k-1

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