Write the balanced chemical equation for the reaction shown here. answer chemistry
1 answer:
I found the attached image with the same statement of your question and think it may be very useful for you that I use it to show how to answer this question (furthermore I think it may be the same reaction that you forgot to include).
As you can see, there are one image on the left side and other image on hte right side of the figure.
Those images contains drawings that represent molecules and a legend that permit you to distinguish the kind of atoms in each molecule.
Using that, you can indicate the chemical reaction as the transformation of the molecules on the left side onto the molecules on the right side:
Left side:
3 molecules of CH4 and 3 molecules of N2Cl4
Right side:
3 molecules of CCl4, 3 molecules of N2 and 6 molecules of H2
That is represented as:
3CH4 + 3 N2Cl4 -----> 3 CCl4 + 3N2 + 6H2
And that is the balanced chemical equation for the reaction shown in the figured attached.
I hope this is useful for you..
As you can see, there are one image on the left side and other image on hte right side of the figure.
Those images contains drawings that represent molecules and a legend that permit you to distinguish the kind of atoms in each molecule.
Using that, you can indicate the chemical reaction as the transformation of the molecules on the left side onto the molecules on the right side:
Left side:
3 molecules of CH4 and 3 molecules of N2Cl4
Right side:
3 molecules of CCl4, 3 molecules of N2 and 6 molecules of H2
That is represented as:
3CH4 + 3 N2Cl4 -----> 3 CCl4 + 3N2 + 6H2
And that is the balanced chemical equation for the reaction shown in the figured attached.
I hope this is useful for you..
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Explanation:
For the given reaction, the temperature of liquid will rise from 298 K to 339 K. Hence, heat energy required will be calculated as follows.
Putting the given values into the above equation as follows.
=
= 1902.81 J
Now, conversion of liquid to vapor at the boiling point (339 K) is calculated as follows.
= energy required =
= latent heat of vaporization
Therefor, calculate the value of energy required as follows.
=
=
= 12121.2 J
Therefore, rise in temperature of vapor from 339 K to 373 K is calculated as follows.
Value of = 1.06 J/g,
= (373 -339) K = 34 K
Hence, putting the given values into the above formula as follows.
=
= 983.892 J
Therefore, net heat required will be calculated as follows.
Q =
= 1902.81 J + 12121.2 J + 983.892 J
= 15007.902 J
Thus, we can conclude that total energy (q) required to convert 27.3 g of THF at 298 K to a vapor at 373 K is 15007.902 J.