Consider the reaction FeO(s)+CO(g) ⇌Fe(s)+CO2(g) for which KP is found to have the following val

Consider the reaction FeO(s)+CO(g) ⇌Fe(s)+CO2(g) for which...

Consider the reaction $\mathrm{FeO}(s)+\mathrm{CO}(g) \rightleftharpoons$ $\mathrm{Fe}(s)+\mathrm{CO}_{2}(g)$ for which $K_{P}$ is found to have the following values: a. Using this data, calculate $\Delta G_{R}^{\circ}, \Delta S_{R}^{\circ},$ and $\Delta H_{R}^{\circ}$ for this reaction at $700 .^{\circ} \mathrm{C}$. Assume that $\Delta H_{R}^{\circ}$ is independent of temperature. b. Calculate the mole fraction of $\mathrm{CO}_{2}(g)$ present in the gas phase at $700 .^{\circ} \mathrm{C}$

Consider the reaction $\mathrm{FeO}(s)+\mathrm{CO}(g) \rightleftharpoons$ $\mathrm{Fe}(s)+\mathrm{CO}_{2}(g)$ for which $K_{P}$ is found to have the following values:
a. Using this data, calculate $\Delta G_{R}^{\circ}, \Delta S_{R}^{\circ},$ and $\Delta H_{R}^{\circ}$ for this reaction at $700 .^{\circ} \mathrm{C}$. Assume that $\Delta H_{R}^{\circ}$ is independent of temperature.
b. Calculate the mole fraction of $\mathrm{CO}_{2}(g)$ present in the gas phase at $700 .^{\circ} \mathrm{C}$

Key Concepts

Standard Gibbs Free Energy and Equilibrium Constant

This concept relates the standard change in Gibbs free energy (?G°) of a reaction to its equilibrium constant (K) through the equation ?G° = -RT ln K. It is a central idea in thermodynamics that bridges measurable equilibrium properties with thermodynamic potentials, allowing one to determine how favorable a reaction is under standard conditions.

Reaction Thermochemistry (?H° and ?S° Relationships)

This concept involves the interrelationship between the standard enthalpy change (?H°), standard entropy change (?S°), and standard Gibbs free energy change (?G°) of a reaction, expressed by the equation ?G° = ?H° - T?S°. When certain assumptions such as a temperature-independent ?H° are made, one can use data at a given temperature to deduce the values of ?H° and ?S°, which are fundamental for understanding the energy profile of the reaction.

Equilibrium Composition of Gaseous Systems

This concept focuses on determining the composition of a gaseous mixture at equilibrium by using partial pressures and mole fractions. In reactions involving gases, the equilibrium constant expressed in terms of partial pressures (Kp) directly relates to the ratio of partial pressures of reactants and products, allowing one to calculate the mole fraction of a specific gas in the mixture. This approach is essential in practical applications where understanding the distribution of species in the gas phase is required.

Transcript

00:01 In the given question we have been provided a reaction that is the reaction of ferrous oxide with carbon monoxide to form ferric or iron metal, okay, plus carbon dioxide gas, okay? so there are two solid in our reaction while there are two gases, okay? so we have to first calculate in part a, delta z for this reaction, delta s for this reaction, reaction and the delta h for this reaction okay now we know we have been provided the equilibrium constant at two different temperature okay we have been provided kp at a temperature of 700 degrees celsius okay so that is in calvin we will convert that by adding plus 273 so that is 973 kelvin and similarly we have a kp value at 1200 degrees celsius to be 0 .310.

01:02 Okay, this is a 200 degrees celsius.

01:05 So, add 273.

01:06 So we will get the temperature to be 1473 kelvin.

01:11 Now we know that the relation between two equilibrium constant at a different temperature.

01:16 Okay.

01:16 So kp1 and kp2, i am referring this as kp1, this as kp2, is equal to delta h of the reaction divided by universal gas constant 1 upon t1 minus 1, sorry, 1 2 minus 1 upon t1.

01:34 Okay.

01:35 Now our t2 and t1 are this.

01:38 Okay, this is our t1 and this is our t2 temperature.

01:42 Kp1 is 0 .688.

01:45 Kp2 is 0 .310.

01:49 That will be equals to delta h reaction.

01:52 R we will be using, we'll have this value.

01:55 Okay.

01:56 So we can use this 8 .314 into 10 to the power minus 3.

02:01 T2 is over 1473, t1 is 973.

02:08 So when we do this calculation, we will get delta h for this reaction 2p equals to minus 19 kilojoule per mole.

02:17 So that is our answer for delta h of this reaction.

02:20 The value of delta g of the reaction for the same temperature, we are calculating the value at 973 kelvin.

02:27 Okay, for part a.

02:28 So, our delta g of this reaction is equals to minus rt, ln, eclobrium constant at 973 kelvin.

02:38 Okay? so our r is 8 .314 into 10 to the power minus 3.

02:44 Our temperature is 973 while our equilibrium constant at this temperature is 0 .688.

02:52 So our delta g will at this temperature will come out to be 3 .03 kilojoule per mole.

02:59 Okay...

Please give Ace some feedback