Consider the reaction:
I2( g) + Cl2( g) ∆ 2 ICl( g)
K
p = 81.9 at...

Question

Consider the reaction:
I2( g) + Cl2( g) ∆ 2 ICl( g)
K
p = 81.9 at 25 °C
Calculate ΔG
rxn for the reaction at 25 °C under each of the
following conditions:
c. PICl = 2.55 atm; PI2 = 0.325 atm; PCl2 = 0.221 atm

Accepted Answer

Hello everyone today. We have the following problem for the following reaction. We have our Casey constant of 124.6 at 30°C. We are being asked to calculate our change in our gifts for energy of the reaction at 30°C when we have the falling concentrations. And so the first thing you do is you want to recall our equation for solving for the gibbs free energy for the reaction. So that's gonna be negative. The gas constant times our temperature time is our natural log of K. So are gas constant is going to be 8. jewels per mole kelvin. Our temperature is 30°C. However, we're going to add to 73.15 because we need this in Kelvin and then we're going to multiply by our natural log of R. K. C. Which is 124.6. And this is going to equal negative 10, 161.15 jewels per mole. So now we have to calculate Q. Because that, is that a normal temperature. However, this is going to be a at this separate point. So we're gonna calculate Q. Which is going to be the concentration of our products over our concentration of reactant. So our products and this equation were B and C. So we're going to put B and brackets. However, we have a two in front of B is the coefficient. So that's going to be raised as an experiment for B. We're gonna multiply that by sea. And then we have our reactant here, which is A And so we're gonna calculate next hour change in our gibbs free energy of the reaction for this one. And so this is going to be calculated by taking the total gibbs free energy that we calculated before and adding it to our gas constant times our temperature times our natural log of Q. And so that's gonna look like this. We're gonna have our negative 12,001, 61.15 jewels per mole plus Our gas constant, which is 8.314, joules per mole, Kelvin times our temperature that we said was 30 degrees of Celsius plus our 2 73.15. And in times our natural log and that's going to be our .25 because that is what B. Is the concentration of B. And that is going to be squared times the concentration of C, which is .18 Over a concentration of a, which is .32. And so through this, we are going to get an answer of negative 20,599. jewels per mole. However, we're gonna need to convert this into killer jewels. So we're gonna use the conversion factor that one kg is equal to 10 to the third jewels. And when our units cancel, we're left with negative 20.6 kg joules per mole as our final answer. Overall, I hope this helped. And until next time

Consider the reaction: I2( g) + Cl2( g) ∆ 2 ICl( g) K p = 81.9 at 25 °C Calculate ΔG rxn for the reaction at 25 °C under each of the following conditions: c. PICl = 2.55 atm; PI2 = 0.325 atm; PCl2 = 0.221 atm

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