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Consider de following reaction at 25∘C :A ⇔ B + C with a ΔG'∘∘=0.0 kJ/molWhat is the value of ΔG when the initial concentration...

Question

Consider de following reaction at 25∘C :A ⇔ B + C with a ΔG'∘∘=0.0 kJ/molWhat is the value of ΔG when the initial concentrations ofA, B, and C 1M and 1x10^-6M?Which concentration will generate Gibbs free energy?

Consider de following reaction at 25∘C : A ⇔ B + C with a ΔG'∘∘=0.0 kJ/mol What is the value of ΔG when the initial concentrations of A, B, and C 1M and 1x10^-6M? Which concentration will generate Gibbs free energy?



Answers

Calculate $\Delta G^{\text {o }}$ for the reaction $A+B \rightleftharpoons C+D$ at $25^{\circ} \mathrm{C}$ when the equilibrium concentrations are $[\mathrm{A}]=10 \mu \mathrm{M},[\mathrm{B}]=15 \mu \mathrm{M},[\mathrm{C}]=$ $3 \mu \mathrm{M},$ and $[\mathrm{D}]=5 \mu \mathrm{M} .$ Is the reaction exergonic or endergonic under standard conditions?

Hello students in this question we have given a reaction for which the change in and therapy delta H. Is 82.8 kg jewel at temperature T equals to 25 C that is 2 98 Calvin. So we have to determine changing internal energy DELTA you. So we know that meant to educate is equal to dental floss dente angie Marie claire by RT. So Delta H. is 80 2.8 kg jewel. This is equal to delta U. Plus N. G. Which is the changing number of moles which can be seen from the occupation is one and our which is 8.3 and four temperature is 2 98 Calvin. And they were by 1000 to convert it into the kalamazoo. So delta you from here after solving He's obtained as 80.3 to kill Jews. Okay so from the given options option B. Here is the correct answer for this problem. Okay thank you.

Here we are continuing with the reactivity and the properties of the main groups from the periodic table of elements. Where the main group is vastly made up of the P. Block, which is the electro negative non metals, as well as the S block, the electro positive metals. So the gibbs, free energy of formation is related to our equilibrium constant where we have delta jean or Is equal to negative 2.303. Rt log K P. So here we'll crack you late K. P. So what we have is 1.70 kg joules per mole. It's equal to negative 2.303, multiplied by 8.314 jules Permal pack, Calvin Multiplied by 2 9, 8 Calvin multiplied by log K. P. When we rearrange the K P. And that is equal to north .999.

Going to calculate the standard entropy for a certain non spontaneous reaction. So the information that we're given is the temperature that the reaction occurs is 50 C, which is also equal to 323 Calvin, which will help for future calculation. And the standard entropy of the reaction is equal to 104 Jules per Kelvin. Since we're looking to calculate RFLP value in killing jewels, let's go ahead and convert our jewels into kill jewels. There's one killer Jewell in 1000 goals. Therefore there's 0.14 killed jewels, Permal, Calvin or per Calvin in this entropy of reaction. Okay, so let's go ahead and write our equation here. We know that our Delta she standard is equal to our standard M v P minus our temperature and standard entropy. So we're given one other piece of information in this reaction. We know that this reaction is non spontaneous when we have a reaction that is non spontaneous. We know that our delta G value here, our delta G value is greater than one. So let's put the pieces of this puzzle together. We know that the there is greater than zero not greater than one. Excuse me. So let's put it these puzzle pieces together. So we know that our adult EGY value has to be positive and we have some numerical values for here. So that's hypothetically. Just say that our Delta G is greater than one is equal to adults. H value minus R T value, which is going to be 323 Calvin times are adults s value, which is 100 4.14 killed jewels for Tillman and we get that are positive. Delta G value is equal to adults age value minus 33 point six Kelly jewels So in this case, we know that our Delta H value must be a positive number that is greater than 33.6 in order for our Delta G value to be positive. Therefore, our Delta H must be greater than positive 33.6 Killer Joel's in order for this reaction to be non spontaneous, therefore, with a positive Delta H value, this reaction is endo thermic and the entropy value for which this reaction has to be has to remain non spontaneous. Will have to be 33.6 killed jewels

Yeah. For this question, we have a chemical reaction of one mall, The hydrogen sulfide reacting with sulphur dioxide, producing three moles, gaseous sulphur and two moles liquid water. Delta H is negative at -233 killer jewels. And Delta S. is also negative at negative for 24 jewels per Kelvin. Because both of these are negative. That indicates that this reaction is spontaneous at low temperatures. If they were both positive, it would suggest that reaction is spontaneous at high temperatures. So let's calculate delta G at 393 Kelvin to do that will take DELTA G is equal to delta H minus T. The temperature 3 93, multiplied by delta S delta S. However, we will convert from jules per kelvin to kill jules per kelvin. So the units are the same when we sum them up to get delta G And we get Delta G equal to negative 66.4 killer jewels. To determine at what temperature is it spontaneous? We first need to determine the temperature at which it said equilibrium, and delta G is equal to zero. To do that will set DELTA G equal to zero, put in our delta H and then minus T delta S. Solve for T. We get 5 50 kelvin, And because both of these are negative, we know that it's spontaneous at low temperatures, so it must be spontaneous at temperatures less than 550 Calvin.


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