Consider the following reaction: 2NH3(8) N2(g) + 3H2(g) If 4.23x10 moles of NH3, 0.213 moles of Nz, and 0.272 moles...
Consider the chemical reaction 2NH3(g) ó N2(g) + 3H2(g). The equilibrium is to be established in a 50.0 L container at 1,000 K, where Kc = 4.0 × 10-2. Initially, 6.10 x 105 moles of NH3(g) are present. Calculate the amount of H2 presentat equilibrium. [H2] =_____
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
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=
Consider the following reaction where K = 0.159 at 723 K: N2(g) + 3H2(g) = 2NH3(g) A reaction mixture was found to contain 4.65*10*2 moles of N2(g), 3.76x10-2 moles of H2(g) and 5.50*10-4 moles of NH3(g), in a 1.00 Liter container Indicate Truc (T) or False (E) for each of the followingi 1. In order to reach equilibrium NH3(g) must be consumed. 2. In order to reach equilibrium K must decrease. 3. In order to reach equilibrium N, must be...
The equilibrium constant, K, for the following reaction is 6.30 at 723K. 2NH3(g) N2(g) + 3H2(g) If an equilibrium mixture of the three gases in a 10.1 L container at 723K contains 0.410 mol of NH3(g) and 0.250 mol of N2, the equilibrium concentration of Hy is M.
Consider the following reaction where K. = 6.30 at 723 K. 2NH3(B) = N2(g) + 3H2() A reaction mixture was found to contain 5.30*10* moles of NH3(g), 4.55*10moles of N2(8), and 3.67x10-2 moles of H2(e), in a 1.00 liter container Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium B. must run in the reverse...
Consider the following reaction where K. = 6.30 at 723 K. 2NH3() N2(g) + 3H2(8) A reaction mixture was found to contain 6.48*10* moles of NH3(g), 2.78 102 moles of N2(e), and 4.23-102 moles of H2(g), in a 1.00 liter container Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the...
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
The equilibrium constant, Kc, for the following reaction is 6.30 at 723K. 2NH3(g) N2(g) + 3H2(g) If an equilibrium mixture of the three gases in a 15.7 L container at 723K contains 0.284 mol of NH3(g) and 0.437 mol of N2, the equilibrium concentration of H2 is__________ M.
Question 5 (1 point) Consider the following reaction at equilibrium: 2NH3(g) N2(g) + 3H2(g) Le Châtelier's principle predicts that the moles of H2 in the reaction container will increase with O a decrease in the total pressure (T constant) some removal of NH3 from the reaction vessel (V and T constant) an increase in total pressure by the addition of helium gas (V and T constant) a decrease in the total volume of the reaction vessel (T constant) addition of...