Answer:
<u>✌</u><u>3</u><u> </u><u>I</u><u> </u><u>think</u><u> </u><u>-</u><u> </u><u>She</u><u> </u><u>should</u><u> </u><u>not</u><u> </u><u>have</u><u> </u><u>multiplied</u><u> </u><u>the</u><u> </u><u>hydrogen</u><u> </u><u>atoms</u><u> </u><u>by</u><u> </u><u>the</u><u> </u><u>coefficient</u><u>. </u><u> </u><u>sorry</u><u> </u><u>im</u><u> </u><u>not</u><u> </u><u>sure</u><u> </u><u>but</u><u> </u><u>I</u><u> </u><u>tried</u><u> </u><u>tell</u><u>,</u><u> </u><u>tell</u><u> </u><u>me</u><u> </u><u>if</u><u> </u><u>im</u><u> </u><u>wrong</u><u> </u><u>Plz</u><u>!</u><u>✌</u>
Explanation:
<em>❤</em><em>So</em><em> </em><em>sorry</em><em> </em><em>if</em><em> </em><em>it's</em><em> </em><em>wrong</em><em>. </em><em>❤</em>
Answer: 438 K
Explanation:
According to Gibbs equation:
= Gibb's free energy change
= enthalpy change = 20.1 kJ/mol = 20100 J/mol
T = temperature
= entropy change = 45.9 J/Kmol
A reaction is at equilibrium when = Gibb's free energy change is zero and becomes spontaneous when = Gibb's free energy change is negative.
T=437.9K
Thus the temperature at which the reaction change from nonspontaneous to spontaneous in the forward direction is 438 K
Answer:
I don't know if this will really help you but I'll try to explain it
Explanation:
it wants you tell some things you see on the graph. Some examples you can say is what kind of bond it is and things like that. You can use a periodic table