Question

For an exothermic dissolving process, predict the signs for the change in enthalpy, entropy, and free energy and explain how temperature will affect these changes. (3 points)

Answer 1

@just_one_last_goodbye @j.youmans @thomaster

Answer 2

@iPwnBunnies

Answer 3

Change is Entropy is \[\Delta S \] right?

Answer 4

i dont know chemistry :/

Answer 5

:(

Answer 6

@SolomonZelman

Answer 7

Really no one can help me with this. -.- OS is never a help for me.

Answer 8

@magbak @Preetha @Whitemonsterbunny17

Answer 9

I will tag all of OS until someone helps me. :(

Answer 10

Last resort :'( @ganeshie8

Answer 11

@PANTIEPOWER

Answer 12

0H no one is helping i guess i better be loved for this give me a second.

Answer 13

hope she is better at chemistry than COD

Answer 14

xD

Answer 15

Ok first thing is j. shush xD and the Your right jr \[\Delta S \] is right.

Answer 16

hey you know its true jess

Answer 17

Is this one of these open ended questions so i can answer accurately. and its not i can beat u j.

Answer 18

Yeah open ended.

Answer 19

sure you can

Answer 20

Ok so in this case with increasing temperature, entropy and enthalpy will remain constant.

Answer 21

she is good at chemistry o_O is the world upside down cause i think it is oppisite day

Answer 22

In an exothermic reaction, heat is given off. What that means is \[Final\] enthalpy should be less than the \[initial\] enthalpy. And since H = Hf - Hi (Hf < Hi), H (enthalpy) should be negative. (-)

Answer 23

Right.

Answer 24

Ok you should also know

\[\Delta H\]is positive as heat is needed to form bonds
\[\Delta S\] is positive as there is a state of physical or chemical changes
\[\Delta G\]is dependent upon temerature

Answer 25

Ur good at this.

Answer 26

:)

Answer 27

Ok so as temperature increases, the free energy will get more and more negative.

You should be able to put your answer together bruh xD.