A student ran the following reaction in the laboratory at 557 K: CO(g) + Cl2(g) =...
A student ran the following reaction in the laboratory at 529 K: CoCl2(g) P CO(g) + Cl2(g) When she introduced 1.68 moles of CoCl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 3.61*10-2 M. Calculate the equilibrium constant, Ke she obtained for this reaction. Kc =
1. A student ran the following reaction in the laboratory at 632 K: 2HI(g) ->H2(g) + I2(g) When she introduced 0.362 moles of HI(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 3.55×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = 2. A student ran the following reaction in the laboratory at 616 K: CO(g) + Cl2(g) -> COCl2(g) When she introduced 0.131 moles of CO(g) and 0.161 moles...
A student ran the following reaction in the laboratory at 541 K: COC12(E) CO(g) + Cl2(g) When she introduced 1.13 moles of COC12(e) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 3.83x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction.
A student ran the following reaction in the laboratory at 425 K: PCl5(g) --> PCl3(g) + Cl2(g) When she introduced 4.59 moles of PCl5(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 3.94×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
A student ran the following reaction in the laboratory at 330 K: 2NO(g) + Br (9) 2 2NOBr(g) When she introduced 0.103 moles of NO(g) and 9.25x10-- moles of Br (9) into a 1.00 liter container, she found the equilibrium concentration of Br2(g) to be 5.67x10-2 M. Calculate the equilibrium constant. Ko she obtained for this reaction. K =|
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 280 K: 2CH2Cl2(g) CH(g) + CC14(8) When she introduced 8.40x10-2 moles of CH,CL2(g) into a 1.00 liter container, she found the equilibrium concentration of CCI,(g) to be 3.93x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction. K=
A student ran the following reaction in the laboratory at 325 K 2NO(8) + Br2(e)2NOBr(g) When she introduced 0.120 moles of NO(g) and 9.52x102 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of Br2(g) to be 5.35x102 M. Calculate the equilibrium constant, Kg, she obtained for this reaction. Ke
A student ran the following reaction in the laboratory at 324 K: 2NO(g) + Br2(g) 2NOBr(g) When she introduced 0.137 moles of NO(g) and 0.119 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of Br2(g) to be 6.92×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
A student ran the following reaction in the laboratory at 254 K: 2NO(g) + Br2(g) ⇌ 2NOBr(g) When she introduced 0.185 moles of NO(g) and 0.130 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.152 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =