5. The following equilbrium partial pressures were measured at some temperature:
NH3 | N2 | H2 |
0.240 atm | 0.290 atm | 0.330 atm |
Determine the value of the equilibrium constant at the temperature of the reaction for the following reaction. Your are given values to 3 significant figures, so make sure you answer to three significant figures to avoid rounding errors in WebAssign.
N2 + 3H2 2NH3
K =
In a different experiment at the same temperture, the equilibrium pressure of N2 was found to be 0.350atm and that of H2 to be 0.240 atm. What is the equilibrium pressure NH3 if K = 6.400 for the above reaction at the temperature of the equilibrium?
P(NH3) = atm
5. The following equilbrium partial pressures were measured at some temperature: NH3 N2 H2 0.240 atm...
The partial pressures of N2, H2, and NH3 were measured as 0.301, 1.00, and 0.0100 atm, respectively, in the reaction shown below. Temperature is 650 K. What is the value of ΔGrxn? (ΔGºrxn = 41.90 kJ) N2(g)+3H2(g)2NH3(g) Kp = 4.3 x 10^−4 FIND ΔGrxn = kJ We were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this image
HQ14.35 Unanswered The reaction mixture N2(g) +3H2(g)2NH3(g) has the following equilibrium partial pressures: PN2- 2.40 atm, PH2-1.60 atm, and PNH3 22.10 atm. Calculate the equilibrium constant Kp. Report your answer to the correct number of significant figures. Type your response
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.
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
18) Calculate the pressure of N2 if the equilibrium pressures of H2 = 2.0 atm, and NH3 = 0.5 atm, and Kp = 2.0 N2(g) + 3 H2(g) = 2 NH3(g) A) 0.031 atm (B).016 atm C) 0.062 atm D) 62,5 atm E) 0.40 atm 19) Consider the following reaction: CH4(g) + 2 H2S(g) = CS2(g) + 4 H2(g)
3. {7} Consider equilibrium N2 (g) + 3 H2(g) 5 2NH3(g) K, -4,51 x10-at 450 °C. For the mixture below indicate the direction of this equilibrium reaction toward product or toward reactants) at the following partial pressures: 105 atm NH3; 35 atm N2; 495 atm H:
Ammonia, NH3(g)NH3(g), at a pressure of 1.13 bar, is placed in a container at a certain temperature. When equilibrium is established at that temperature, the pressure of H2(g)H2(g) is 0.620 bar. Part A Determine the value of KPKP for the decomposition of NH3NH3 at that temperature: 2NH3(g)⇌3H2(g)+N2(g)2NH3(g)⇌3H2(g)+N2(g) Express your answer in squared bars to three significant figures. Please show steps and the final units in bar^2
N2(g) + 3 H2(g) ⇌ 2 NH3(g) KP = 6.78 x 105 at 298 K (determined using atm) A 7.5 x 101 L container being held at 298 K is charged with the three gases present in the above equation. Once finished, the initial partial pressure of N2 was 0.59 atm, the initial partial pressure of H2 was 0.45 atm, and the initial partial pressure of NH3 was 0.11 atm. The gas mixture was then allowed to reach equilibrium. Use...
At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches equilibrium when the partial pressures of nitrogen, hydrogen, and ammonia gases are 4.00 atm, 1.00 atm, and 1.05 x 10−2 atm, respectively. Given that the standard enthalpy of the reaction at 400K is DH = -94 kJ/mol, estimate the value of the equilibrium constant KP at 450 K assuming that the standard enthalpy of reaction does not vary significantly with temperature in this temperature...
For the reaction 2NH3(g)<->N2(g)+3H2(g), Kc=0.0076 at a particular temperature. If 0.025 M NH3, 0.50M N2, and 0.015 M H2 are mixed in a reaction vessel, is the reaction at equilibrium? If not, in what direction will the reaction shift to reach equilibrium?