Comment in case of any doubt.
For the reaction below the partial pressure of NO: is 0.25 atm and the partial pressure of N:O. is 1.0 atm. What is...
0.25/1 EARNED 27 An equilibrium is established for the reaction 2 CO(g) + MOD (s) – 2 CO (9) + Moisi. a Which of the following is the correct expression for Kp? > 0.25 of 0.25 points earned Lse the expression for Kp from part a. If at equilibrium the partial pressure of carbon monoxide is 5 21 atm and the partial pressure of the carbon dioxide is 0.721 atm, then what is the value of ko? b > of...
What is the equilibrium partial pressure of methane, PCH4 in the reaction that follows given that the equilibrium partial pressure of hydrogen, PH2 = 1.22 atm and Kp = 0.262 at 1000 oC? C (s) + 2 H2 (g) -> CH4 (g Answer Choices: 1. PCH4 = 0.320 atm 2. PCH4 = 0.390 atm 3. PCH4 = 0.565 atm 4. PCH4 = 4.66 atm 5. PCH4 = 5.68 atm
Consider the reaction below SO(0) + NOz(a) SO,(a) + NO(g) K = 0.25 at 900 °C If p802 4.0 atm, p803 - 1.0 atm, PNO 1.0 atm at a given point in time, what is the equilibrium partial pressure of so m ? Give your answer in 2 significant figures
. Calculate the partial pressure of H2(g) at equilibrium for the following reaction at 90.0°C if the partial pressure of C2H2(g) is 1.8 atm and the partial pressure of C2H6(g) is 0.30 atm. C2H2(g) + 2H2(g) ⇄ C2H6(g) KP = 0.045
Consider the following reaction: A(g)?2B(g) Find the equilibrium partial pressures of A and Bfor each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions. Kp= 1.8 Kp= 1.6×10?4 Kp= 1.8×105
Consider the following reaction: A(g)⇌2B(g) Find the equilibrium partial pressures of A and Bfor each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions. A.)Kp= 2.0 B.) Kp= 1.6×10−4 C.)Kp= 1.4×105
Consider the following reaction: A(g)⇌2B(g) Find the equilibrium partial pressures of A and B for each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions. 1.PA, PB, Kp= 1.4 2.PA, PB, Kp= 1.8×10^−4 3.PA, PB, Kp= 2.0×10^5
Consider the reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) Kp=2.91×103 at 298 K In a reaction at equilibrium, the partial pressure of SO2 is 0.156 atm and that of Cl2 is 0.365 atm . What is the partial pressure of SO2Cl2 in this mixture?
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(g) 2 NO ( g ) + O 2 ( g ) ↽ − − ⇀ 2 NO 2 ( g ) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol Δ G ° = − 72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.300 atm P NO...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N 2 ( g ) + 3 H 2 ( g ) − ⇀ ↽ − 2 NH 3 ( g ) the standard change in Gibbs free energy is Δ G ° = − 32.8 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are P N 2 = 0.100 atm...