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Consider the following reaction: 2HI(g) =H2(g) +12(9) If 1.87 moles of HI, 0.333 moles of H2,...
The equilibrium constant, Kp, for the following reaction is 1.80x10-2 at 698K. 2HI(g) =H2(g) +12(g) If an equilibrium mixture of the three gases in a 14.3 L container at 698K contains HI at a pressure of 1.09 atm and H, at a pressure of 0.929 atm, the equilibrium partial pressure of I, is atm. Submit Answer Retry Entire Group 9 more group attempts remaining
Consider the following reaction where K, 55.6 at 698 K: H2(8) +12(8) 2HI(g) A reaction mixture was found to contain 4.76x102 moles of H2(8), 3.98x102 moles of I(8) and 0.295 moles of HI(g), in a 1.00 Liter container Indicate True (T) or False (E) for each of the following: 1. In order to reach equilibrium HI(g) must be produced 2. In order to reach equilibrium Kmust decrease 3. In order to reach equilibrium Hy must be consumed 4., is greater...
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...
The equilibrium constant for the following reaction is 1.80x102 at 698K 2HI(8)H2( ) +I2(g) If an equilibrium mixture of the three gases at 698K contains 2.35x102 M HI(g) and 2.63x10-2 M H, what is the equilibrium concentration of I? Submit Answer Retry Entire Group 9 more group attempts remaining
The equilibrium constant, K, for the following reaction is 55.6 at 698 K. H2(g) + 12 (g) = 2 HI(g) Calculate the equilibrium concentrations of reactants and product when 0.262 moles of H2 and 0.262 moles of 12 are introduced into a 1.00 L vessel at 698 K. Σ [H2) = [12] = [HI] = Σ Σ Submit Answer Retry Entire Group 9 more group attempts remaining
A student ran the following reaction in the laboratory at 684 K: H2(g) + 12(g) 22HI(g) When she introduced H2(g) and Iz() into a 1.00 L evacuated container, so that the initial partial pressure of H2 was 4.88 atm and the initial partial pressure of I was 3.74 atm, she found that the equilibrium partial pressure of 12 was 0.465 atm. Calculate the equilibrium constant, Kp. she obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more...
Consider the following reaction where Kp = 55.6 at 698 K: H2(g) +12(g) 22HI(g) If the three gases are mixed in a rigid container at 698 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following: 1. A reaction will occur in which HI(g) is produced. 2. Kp will decrease. 3. A reaction will occur in which Hy is consumed. 4. Q is...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2 (g) + 12 (g) = 2 HI(g) Calculate the equilibrium concentrations of reactants and product when 0.286 moles of H2 and 0.286 moles of 12 are introduced into a 1.00 L vessel at 698 K. M [H2) = [12] = [HI]= M M Submit Answer Retry Entire Group 9 more group attempts remaining
Consider the following reaction: 2 HI(g) H2(g) + I2(g) If 2.29 moles of HI, 0.309 moles of H2, and 0.363 moles of I2 are at equilibrium in a 17.8 L container at 774 K, the value of the equilibrium constant, Kp, is
The equilibrium constant, Kfor the following reaction is 1.55x0 at 644 When a sufficientiy large sample of HI(g) is introduced into an evacuated vessel at 644 K, the equilibrium concentration of I2)s found to be 0.303 M Calculate the concentration of HI in the equilibrium mixture. more group attempts remaining Submit Anawer Retry Entire Group Consider the following reaction where K 0.159 at 723 K. A reaction mixture was found to contain 2.07x102 moles of N2), 4.45x10-2 moles of H2)...