At 25 °C the reaction from Part A has a composition as shown in the table...
At 25 ?C the reaction from Part A has a composition as shown in the table below. Substance Pressure (atm) C2H2(g) 3.75 H2(g) 4.75 C2H6(g) 5.25×10?2 What is the free energy change, ?G, in kilojoules for the reaction under these conditions?
Part B At 25 ∘C the reaction from Part A has a composition as shown in the table below. Substance Pressure (atm) C2H2(g) 4.75 H2(g) 3.45 C2H6(g) 4.25×10−2 What is the free energy change, ΔG, in kilojoules for the reaction under these conditions?
At 25 ∘C the reaction from Part A has a composition as shown in the table below. Substance Pressure (bar) C2H2(g) 4.45 H2(g) 5.65 C2H6(g) 3.25×10−2 What is the Gibbs energy change, ΔrG, in kilojoules per mole for the reaction under these conditions? Express your answer numerically in kJ mol−1.
I solved A but I'm confused on how to solve B if someone could please help me I would highly appreciate it Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is C2H2(g) + 2H2(g) = C2H6(g) Given the following data at standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K), what is the value of Kp for this reaction? Substance AG: (kJ/mol) 209.2 C2H2(g) H2(g) C2H6(g)...
Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is C2H2(g)+2H2(g)⇌C2H6(g) At 25 ∘C the reaction from ^ has a composition as shown in the table below. Substance Pressure (atm) C2H2(g) 5.35 H2(g) 5.75 C2H6(g) 5.25×10−2 What is the free energy change, ΔG, in kilojoules for the reaction under these conditions? Express your answer numerically in kilojoules.
In Part A, we saw that ΔG∘=−242.1 kJ for the hydrogenation of acetylene under standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K). In Part B, you will determine the ΔG for the reaction under a given set of nonstandard conditions. At 25 ∘C the reaction from Part A has a composition as shown in the table below. Substance Pressure (atm) C2H2(g) 3.75 H2(g) 4.25 C2H6(g) 5.25×10−2 What is the free energy change, ΔG,...
The equilibrium constant of a system, K, can be related to the standard free energy change, ΔG∘ ΔG∘=−RTlnK where T is a specified temperature in kelvins (usually 298 KK) and R is equal to 8.314 J/(K⋅mol) Under conditions other than standard state, the following equation applies: ΔG=ΔG∘+RTlnQ In this equation, Q is the reaction quotient and is defined the same manner as KK except that the concentrations or pressures used are not necessarily the equilibrium values. Part A Acetylene, C2H2,...
Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is C2H2(g)+2H2(g)?C2H6(g) Given the following data, what is the value of Kp for this reaction? Substance ?G?f (kJ/mol) C2H2(g) 209.2 H2(g) 0 C2H6(g) ?32.89 In Part A, we saw that ?G?=?242.1 kJ for the hydrogenation of acetylene under standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K ). In Part B, you will determine the ?G for the...
For the reaction 2C(s) + H2(g) + C2H2(g); AG° = 209.2 kJ/mol at 25 °C. If the initial conditions of the reaction are: P(H2) = 128 atm and P(C2H2) = 0.0023 atm, determine the value of AG for the reaction.
Calculate the free energy AG at 25°C for the nonstandard conditions at point where the reaction quotient Q is 2.75 x 10 Express your answer numerically in kilojoules. View Available Hint(s) % ALC O ? AG - CO Nitrosyl chloride formation Chlorine gas. Cl(s), reacts with nitric oxide, NO(), to form nitrosyl chloride, NOCI(g), via the reaction Cl(s) + 2NO(g) + 2NOCI() The thermodynamic data for the reactants and products in the reaction are given in the following table: Substance...