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A student ran the following reaction in the laboratory at 672 K 2NH3(g) = N2(g) +...
A student ran the following reaction in the laboratory at 745 K: N2(g) + 3H2(g) 2NH3(g) When she introduced 3.44x10-2 moles of N2(g) and 5.80x10-2 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 7.82x10-4M. Calculate the equilibrium constant, K., she obtained for this reaction. K=
A student ran the following reaction in the laboratory at 651 K: 2NH3(g)N2(g) + 3H2(g) When she introduced 7.88x102 moles of NH (g) into a 1.00 liter container, she found the equilibrium concentration of NH (g) to be 6.75x103 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc
A student ran the following reaction in the laboratory at 691 K: N2(g) + 3H2(g) 2NH3(g) When she introduced 3.69x10-2 moles of N2(g) and 6.11x10-2 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of H2(8) to be 5.87*10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Ko
A student ran the following reaction in the laboratory at 312 K: 2NO(g) + Br2(g) 2NOBr(g) When he introduced NO(g) and Br2(g) into a 1.00 L evacuated container, so that the initial partial pressure of NO was 1.07 atm and the initial partial pressure of Br2 was 0.448 atm, he found that the equilibrium partial pressure of Br2 was 0.189 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp =
A student ran the following reaction in the laboratory at 662 K: 2NH3(g) N2(s)+3H2(g) When she introduced 6.54x10 9.18x102 M. moles of NH (g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be Calculate the equilibrium constant, K, she obtained for this reaction. 9 more group attempts remaining Submit Answer Retry Entire iroup
A student ran the following reaction in the laboratory at 690. K: H2(g) +12(g) 22HI(g) When he introduced H2(g) and 12(g) into a 1.00 L evacuated container, so that the initial partial pressure of H2 was 4.40 atm and the initial partial pressure of I was 3.28 atm, he found that the equilibrium partial pressure of HI was 5.78 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more group...
A student ran the following reaction in the laboratory at 677 K: 2HI(g) H_2(g) + I_2(g) When she introduced HI(g) at a pressure of 5.32 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of HI(g) to be 4.22 atm. Calculate the equilibrium constant, K_p, she obtained for this reaction. K_p =
A student ran the following reaction in the laboratory at 479 K PC13(E) + Cl2) PC (e) When she introduced PCIy(R) and Cl() into a 1.00 L evacuated container, so that the initial partial pressure of PCI, was 2.39 atm and the initial partial pressure of Cl; was 1.94 atm, she found that the equilibrium partial pressure of Cl, was 0.373 am Calculate the equilibrium constant, Ky she obtained for this reaction.
1. A student ran the following reaction in the laboratory at 304 K: 2NO(g) + Br2(g) 2NOBr(g) When she introduced NO(g) and Br2(g) into a 1.00 L evacuated container, so that the initial partial pressure of NO was 1.22 atm and the initial partial pressure of Br2 was 0.574 atm, she found that the equilibrium partial pressure of Br2 was 0.246 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp =
A student ran the following reaction in the laboratory at 494 K: PC13(g) =PC13(g) + C12(E) When she introduced PCI3(g) at a pressure of 0.778 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of Cl2(g) to be 0.387 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр