9. -/0.1 points 0/4 Submissions Used Gaseous NH3 is placed in a closed container at 78...
9. -10.1 points 0/4 Submissions Used Gaseous SO3 is placed in a closed container at 560 °C, where it partially decomposes to SO2 and 02: 2 503(9) = 2 502(9) + 1 02(9) At equilibrium it is found that p(SO3) = 0.006960 atm, P(SO2) = 0.006580 atm, and p(O2) = 0.004150 atm. What is the value of Kp at this temperature? Kp =
Gaseous BrCl is placed in a closed container at 2054 oC, where it partially decomposes to Br2 and Cl2: 2 BrCl(g) 1 Br2(g) + 1 Cl2(g) At equilibrium it is found that p(BrCl) = 0.004430 atm, p(Br2) = 0.008780 atm, and p(Cl2) = 0.002480 atm. What is the value of KP at this temperature? We were unable to transcribe this imageGaseous Brel is placed in a closed container at 2054 °C, where it partially decomposes to Br2 and Cl2: 2...
Gaseous NOBr is placed in a closed container at -165 oC, where it partially decomposes to NO and Br2: 2 NOBr(g) 2 NO(g) + 1 Br2(g) At equilibrium it is found that p(NOBr) = 0.003400 atm, p(NO) = 0.005450 atm, and p(Br2) = 0.007050 atm. What is the value of KP at this temperature? KP = ______
Gaseous BrCl is placed in a closed container at 1099 oC, where it partially decomposes to Br2 and Cl2: 2 BrCl(g) 1 Br2(g) + 1 Cl2(g) At equilibrium it is found that p(BrCl) = 0.002670 atm, p(Br2) = 0.004740 atm, and p(Cl2) = 0.004780 atm. What is the value of KP at this temperature? KP = .
Gaseous NOBr is placed in a closed container at -171 °C, where it partially decomposes to NO and Br: 2 NOBr(g)# 2 NO(g) + 1 Br2(g) At equilibrium it is found that p(NOBr) 0.007190 atm, p(NO) - 0.009050 atm, and p(Br2) 0.003760 atm. What is the value of Kp at this temperature? Ko
Gaseous hydrogen iodide is placed in a closed container at 425 ∘C, where it partially decomposes to hydrogen and iodine: 2HI(g)←−→H2(g)+I2(g). At equilibrium it is found that [HI]= 3.58×10−3 M , [H2]= 4.86×10−4 M , and [I2]= 4.86×10−4 M . What is the value of Kc at this temperature?
My Notos Gaseous NO is placed in a dlosed container at 509 "C, where it partially decomposes to NO and NO 3 NO(g)1 NO(g) + 1 N0(g) At equilibrium it is found that p(NO)- 0.009570 atm, p(NO ) - 0.005240 atm, and p(N-O) - o.004640 atm, What is the value of K at this temperature? Ke
15. + -10.1 points 0/4 Submissions Used Calculate the standard enthalpy of formation of gaseous nitrogen monoxide (NO) using the following thermochemical information: N2(g) + 3 H2(g) = 2 NH3(9) 4 NO(g) + 6 H2O(l) = 4 NH3(g) + 5 O2(9) 2 H2O(1) = 2 H2(g) + O2(9) AH = -92.4 kJ AH = +1167.1 kJ AH = +571.7 kJ AH =
10. + -/0.1 points 0/4 Submissions Used At 2177 °C the equilibrium constant for the reaction: 2 BrCI(9) = Br2(9) + Cl2(9) is Kp = 1.03. If the initial pressure of Brc is 0.00616 atm, what are the equilibrium partial pressures of BrCl, Br2, and Cl2? P(BrCI) = P(Br2) = p(Cl2) =
10. -/0.1 points 0/4 Submissions Used At 6412 °C the equilibrium constant for the reaction: 2 NO(O) = N() + O2(a) is Kp - 1.32. If the initial pressure of NO is 0.00381 atm, what are the equilibrium partial pressures of NO, N2, and 022 p(NO) - P(N) - (0) -