Answer:
The dissociation of is as follows.
Explanation:
<u>Molecular equation:</u>
In a molecular equation, reactants are present in the molecular form rather than ionic form.
<u>Complete ionic equation:</u>
An ionic equation shows the complete ions in the solution.
<u>Net ionic equation:</u>
A reaction shows only those ions are participating in the reaction.
The dissociation of is as follows.
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Answer:
Answer for the question:
You replicate the CEC analysis of a secondary alcohol you performed in the lab using a reverse phase TLC plate producing the TLC plate below. Based on this TLC plate and the mnemonic in your notes, what can you conclude about the stereochemistry of the alcohol? (1 pts)
is given below which explains the best option for the answer.
Explanation:
The enantiomer of the alcohol cannot be determined.
The U-235 fission will produce krypton-92 and barium-141. And this process will also release huge amount energy. And U-235 also go through α decay model.
Answer:
The answer is NH3 and CH3OH
Explanation:
The basic rule of a reaction is "like dissolves like" and for a homogenous mixture to form, there must be some common properties related to bonding.
1. KI and Hg
Normally mercury tends to form amalgam which is not a homogeneous solution.
2. LICL and C6H14
One is non polar and other is polar which makes the homogeneous reaction not possible.
3. C3H8 and C2H5OH
Both are miscible but will not develop homogeneous solution as propane is gas at normal temperature.
4. F2 and PF3
Flourine is highly electronegative and will repel fellow flourine making it not possible for homogeneous solution
5. NH3 and CH3OH
Both have same type of bonding and can react homogeneously.
Answer:
k = 2.647 x 10-2 M-2 s-1
Explanation:
2NO(g) +Cl2(g) --> 2NOCl(g)
Experiment [NO] (M) [Cl2] (M) Rate (M/s)
1 0.0300 0.0100 3.4 x 10-4
2 0.0150 0.0100 8.5 x 10-5
3 0.0150 0.0400 3.4 x 10-4
Frrom experiments 1 and 3;
Reducing the concentration of NO by a factor of 2 decreases the rate of the reaction by a factor of 4. This means the reaction is second order with respect to NO.
From experiments 2 and 3:
Increasing the concentration of Cl2 by a factor of 4 increases the rate by a factor of 4. This means the reaction is first order with respect to Cl2
The rate equation is given as;
Rate = k [NO]² [Cl2]
From experiment 1;
k = [NO]² [Cl2] / Rate
k = 0.0300² * 0.0100 / 3.4 x 10-4
k = 2.647 x 10-2 M-2 s-1