Ammonia and table salt dissolves in polar solvents, so A is water,
CO2 and hexane are non-polar substances, so they are going to be dissolved in non-polar solvent, so I think it is going to be carbon tetrachloride
Answer is <span>A) A - water; B - carbon tetrachloride
Table salt does not dissolve in oil and CCl4, and Br2 is too active and it is going to react with NH3.</span>
Answer:
C-attracted.
Explanation:
When two magnets stay together they are being attracted. If they are pushing each other away, they are being repelled.
<span>Glycerol is a sub-unit molecule of a Lipid
So, option C is your answer.
Hope this helps!
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The question is incomplete. The complete question is :
A common "rule of thumb" for many reactions around room temperature is that the rate will double for each ten degree increase in temperature. Does the reaction you have studied seem to obey this rule? (Hint: Use your activation energy to calculate the ratio of rate constants at 300 and 310 Kelvin.)
Solutions :
If we consider the activation energy to be constant for the increase in 10 K temperature. (i.e. 300 K → 310 K), then the rate of the reaction will increase. This happens because of the change in the rate constant that leads to the change in overall rate of reaction.
Let's take :
The rate constant = respectively.
The activation energy and the Arhenius factor is same.
So by the arhenius equation,
and
Given, J/mol
R = 8.314 J/mol/K
∴
So, no this reaction does not seem to follow the thumb rule as its activation energy is very low.