The equilibrium constant for this expression is
49.68
HQ14.35 Unanswered The reaction mixture N2(g) +3H2(g)2NH3(g) has the following equilibrium partial pressures: PN2- 2.40 atm,...
For: N2(g) + 3H2(g) ⬄ 2NH3(g), Kp = 4.72 x 10–4 at 475 oC. At equilibrium at 475 oC, PH2 = 0.237 atm and PN2 = 0.582 atm. What is the partial pressure of ammonia at equilibrium?
AGº is -32.7 kJ/mol of N2 for the reaction N2 (g) + 3H2 (g) = 2NH3(g) This calculation was for the reaction under standard conditions—that is, with all gases present at a partial pressure of 1 atm and a temperature of 25°C. Calculate AG for the same reaction under the following nonstandard conditions: . PN2 = 2.00 atm, PH2 = 7.00 atm, PNH3 = 0.021 atm, . and T = 100°C.
KP = 1.000 x 10–4 for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). The reaction is at equilibrium when PH2 = 4.00 atm, PN2 = 4.00 atm, and PNH3 = 0.16 atm. a) Show that these are equilibrium concentrations. b) If the pressure of the system is doubled (the pressure of each gas doubles), what is the final pressure of each gas when equilibrium is restored? If making and using ammonia is important to feeding the world's growing population but...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N2 (g) + 3H2(g) -------> 2NH3(g) the standard change in Gibbs free energy is ΔG° = -72.6 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are PN2 = 0.200 atm PH2 = 0.350 atm PNH3 = 0.850
For the equilibrium 2PH3(g) ⇌ P2(g) +3H2(g), the equilibrium partial pressures are PPH3=0.049 atm, PP2=0.498 atm, and PH2=0.776 atm at 738K. Calculate Kp.
Please explain!
Consider the following reaction N2(g)3H2(g)2NH3(9) Report all answers to three significant figures! a) Determine the standard free energy of the the reaction at 298K AG 33 b) Determine the equilibrium constant at 298K? K-1450x c) Determine the reaction quotient when the partial pressures of the gases are the following N26.70 atm; H2 11.00 atm; NH3 2.30 atm d) Determine the value of ?G when the reaction mixture is the one described in Part C. AG
8. (3 points) Consider the following reaction: N2 (g) +3H2 (g) 2NH3 (g). Find the desired values given the following conditions: PNH3 2.00 atm, PN2 2.00 atm, and PH2 -2.50 atm. The AGo -33.3 kJ/mol at 25 °C. Calculate the Q value for these conditions. a. b. Calculate the AG value for these conditions. c. Is the reactions more or less spontaneous under these conditions compared to the standard conditions? How do you know?
A mixture of gases contains 1.26 g of N2, 3.71 g of H2, and 1.87 g of NH3. If the total pressure of the mixture is 1.67 atm, what is the partial pressure of each component? PN2 = ? atm PH2 = ? atm PNH3 = ? atm
A mixture of gases contains 1.26 g of N2, 8.57 g of H2, and 7.28 g of NH3. If the total pressure of the mixture is 1.66 atm, what is the partial pressure of each component? PN2 = atm PH2 = atm PNH3 = atm
An evacuated (.e. empty) vessel is charged with 84.9 atm of NH3 (g). The following reaction proceeds to reach equilibrium. 2NH3(g) = N2(g) + 3H2(g) At equilibrium, the partial pressure of H2 remains constant at 64.3 atm. The value of Kp is Report your answer to 3 significant figures. Use scientific notation, i.e. 1.23E4.