A student ran the following reaction in the laboratory at 662 K: 2NH3(g) N2(s)+3H2(g) When she...
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 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 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
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box in the reaction equation is an equilibrium sign.
ulat... 2req A student ran the following reaction in the laboratory at 726 K: ration ion ion N2(g)+3H2(g) 2NH3(g) ion When she introduced 3.30x 10-2 moles of N2(g) and 6.61x102 moles of H2(g) into a 1.00 liter container, pulati... M) M) ng Eq... she found the equilibrium concentration of H2(g) to be 6.44x102 M ibri... 2req Calculate the equilibrium constant, Kç, she obtained ng Eq... for this reaction tio... 2req...
Use the References to access impertant values if needed for this question. A student ran the following reaction in the laboratory at 700 K N2(g)+3H2(g) 2NH,(g) When she introduced 3.63x102 moles of N;(g) and 5.18x10 2 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NHs(g) to be 1.11x10 3 M. Calculate the equilibrium constant, Ke, Sshe obtained for this reaction. Ke= Submit Answer Retry Entire Group 7 more group attempts remaining
A student ran the following reaction in the laboratory at 672 K 2NH3(g) = N2(g) + 3H2(8) When he introduced NH3(g) at a pressure of 0.722 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of NH3(g) to be 8.99x103 atm. Calculate the equilibrium constant, Ky, he obtained for this reaction Rp
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 686 K: H2(g) + I2(g) 2HI(g) When she introduced 0.200 moles of H2(g) and 0.230 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.18×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?
A student ran the following reaction in the laboratory at 673 K: H2(g) + I2(g) 2HI(g) When she introduced 0.228 moles of H2(g) and 0.256 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.53×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
A student ran the following reaction in the laboratory at 647 K: 2HI(g) H2(g) + I2(g) When she introduced 0.395 moles of HI(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 3.95×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.