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![2NH3 (g) = N₂ (g) + 3 H2ly) Kp = {PN₂] [ Png ] [P Nha 12 1.5x103: 6.10 )* (0.15) (Pony] (PNH)² = 2.25x10] PNky. (2.25 x 10-7)](http://img.homeworklib.com/questions/a2e0bc60-72ef-11ea-b000-5bcfff795304.png?x-oss-process=image/resize,w_560)
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6. The decomposition of ammonia is: 2 NH (8) N2(8) 400 °C, what is the partial...
7. A solution is prepared by dissolving 0.050 moles of diiodocyclohexane, C&H1012(8), in the solvent CCL....
7. A solution is prepared by dissolving 0.050 moles of diiodocyclohexane, C&H1012(8), in the solvent CCL. The total solution volume is 1.00L. When the reaction: C6H1012 = CH10 + 12 mol has come to equilibrium at 35 °C, the concentration of I, is 0.0350 ! (a) Calculate the concentrations of CeHol, and CeHo at equilibrium. (b) Calculate the equilibrium constant K.
The decomposition of ammonia gas is endothermic, AH = 92 kJ/mol. 2 NH3() = N2(g) +...
The decomposition of ammonia gas is endothermic, AH = 92 kJ/mol. 2 NH3() = N2(g) + 3H2(g) What change to an equilibrium mixture of this reaction will result in the formation of more hydrogen gas? The addition of a catalyst. An decrease in temperature. An increase in volume. A decrease in the concentration of ammonia.
The Haber process { 2 N2(g) + 3 H2(g) <-> 2 NH3(g) } has a Kp...
The Haber process { 2 N2(g) + 3 H2(g) <-> 2 NH3(g) } has a Kp of 4.34 x 10^−3 at 300 K. Calculate the pressure of ammonia that is present at equilibrium if we start with 10 atm of nitrogen and 20 atm of hydrogen gas. Predict whether this concentration would increase or decrease if the original mixture was contained in a 5 L metal bottle and the mixture was allowed to expand into a second 5 L bottle,...
At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches...
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...
At 380 C, the half-life period for the first order decomposition of HO, is 360 min....
At 380 C, the half-life period for the first order decomposition of HO, is 360 min. The energy of activation of the reaction is 200 kJ mor. Calculate the time required c) for 75% decomposition at 450°C. (10 Marks) A mixture of diatomic nitrogen and diatomic hydrogen gas in a 1:3 molar ratio was passed over a catalyst to form ammonia at 450 C. At pressure of 10.13 atm, there was 2.04% by volume of ammonia gas formed. Determine the...
1) a) The decomposition of ammonia is: 2 NHgN(g) +3 H2(g). If the pressure of ammonia...
1) a) The decomposition of ammonia is: 2 NHgN(g) +3 H2(g). If the pressure of ammonia is 1.0 x 10-3 atm, and the pressures of N2 and H2 are each 0.20 atm what is the value for K at 400°C for the reverse reaction? d) What is the [CH&COrVICH:CO,H] ratio necessary to make a buffer solution with a pH of 4.44? K 1.8 x 103 for CH3CO2H. What is the pH of a buffer system prepared by dissolving 10.70 grams...
12) The equilibrium constant, Kp, is 4.51x10 at 450°C for the reaction represented below. N2(g) +...
12) The equilibrium constant, Kp, is 4.51x10 at 450°C for the reaction represented below. N2(g) + 3 H2(g) 2 NH3(g) a. Write the equilibrium expression, Kp, for the reaction. b.Suppose y ou start out with only reactants in a rigid container. The initial partial pressure of N2(g) is 1.0 atm and that of H2(g) is 1.4 atm. What are the partial pressures of each species when the system reaches equilibrium? c. Find K, for this process at 450°C.
1. The reaction N2 + 3 H2 2NH3 is used to produce ammonia. When 450. g of hydrogen...
1. The reaction N2 + 3 H2 2NH3 is used to produce ammonia. When 450. g of hydrogen is reacted with nitrogen, 2550 g of ammonia should be produced. If a chemist actually obtains 1,977 g of ammonia in the lab, what is the percent yield of this reaction? Report your answer to the correct degree of certainty. Do not included units (% yield is understood). 2.Calculate the volume of 2.12 moles of nitrogen gas at temperature of 31.7 oC and a pressure of...
6. In this experiment 2.00 mols of NOCI are placed in a 1.00L equilibrium is achieved,...
6. In this experiment 2.00 mols of NOCI are placed in a 1.00L equilibrium is achieved, nitrogen monoxide NO and chlorine gas equilibrium concentration of NO is 0.66 M. Calculate Kc for this placed in a 1.00 L flask @ 298 K. After ad chlorine gas Cl, form. The alculate Kc for this equilibrium reaction: ? 2 NOCI (g) = 2 NO(g) + Cl2 (8) 3. eaction vessel is charged with hydrogen iodide and heated in a sealed tube to...
please show all work thanks B. Consider the system N2 (9) 3H2 (g) 2 NHs (9) dbie of NHs was placed in a 2.000 liter...
please show all work
thanks
B. Consider the system N2 (9) 3H2 (g) 2 NHs (9) dbie of NHs was placed in a 2.000 liter flask at 25°C. When equilibrium at that temperature, it was determined that the ammonia was reduced A 2.568-g sample was reached N to 75.0% of its original value. 1. Calculate K for the decomposition of 2.00 moles of ammonia at 25.0°C. 2. Calculate K for the decomposition of 2.00 moles of ammonia at NH3 is...
7. A solution is prepared by dissolving 0.050 moles of diiodocyclohexane, C&H1012(8), in the solvent CCL. The total solution volume is 1.00L. When the reaction: C6H1012 = CH10 + 12 mol has come to equilibrium at 35 °C, the concentration of I, is 0.0350 ! (a) Calculate the concentrations of CeHol, and CeHo at equilibrium. (b) Calculate the equilibrium constant K.
The decomposition of ammonia gas is endothermic, AH = 92 kJ/mol. 2 NH3() = N2(g) + 3H2(g) What change to an equilibrium mixture of this reaction will result in the formation of more hydrogen gas? The addition of a catalyst. An decrease in temperature. An increase in volume. A decrease in the concentration of ammonia.
At 380 C, the half-life period for the first order decomposition of HO, is 360 min. The energy of activation of the reaction is 200 kJ mor. Calculate the time required c) for 75% decomposition at 450°C. (10 Marks) A mixture of diatomic nitrogen and diatomic hydrogen gas in a 1:3 molar ratio was passed over a catalyst to form ammonia at 450 C. At pressure of 10.13 atm, there was 2.04% by volume of ammonia gas formed. Determine the...
1) a) The decomposition of ammonia is: 2 NHgN(g) +3 H2(g). If the pressure of ammonia is 1.0 x 10-3 atm, and the pressures of N2 and H2 are each 0.20 atm what is the value for K at 400°C for the reverse reaction? d) What is the [CH&COrVICH:CO,H] ratio necessary to make a buffer solution with a pH of 4.44? K 1.8 x 103 for CH3CO2H. What is the pH of a buffer system prepared by dissolving 10.70 grams...
12) The equilibrium constant, Kp, is 4.51x10 at 450°C for the reaction represented below. N2(g) + 3 H2(g) 2 NH3(g) a. Write the equilibrium expression, Kp, for the reaction. b.Suppose y ou start out with only reactants in a rigid container. The initial partial pressure of N2(g) is 1.0 atm and that of H2(g) is 1.4 atm. What are the partial pressures of each species when the system reaches equilibrium? c. Find K, for this process at 450°C.
6. In this experiment 2.00 mols of NOCI are placed in a 1.00L equilibrium is achieved, nitrogen monoxide NO and chlorine gas equilibrium concentration of NO is 0.66 M. Calculate Kc for this placed in a 1.00 L flask @ 298 K. After ad chlorine gas Cl, form. The alculate Kc for this equilibrium reaction: ? 2 NOCI (g) = 2 NO(g) + Cl2 (8) 3. eaction vessel is charged with hydrogen iodide and heated in a sealed tube to...
please show all work
thanks
B. Consider the system N2 (9) 3H2 (g) 2 NHs (9) dbie of NHs was placed in a 2.000 liter flask at 25°C. When equilibrium at that temperature, it was determined that the ammonia was reduced A 2.568-g sample was reached N to 75.0% of its original value. 1. Calculate K for the decomposition of 2.00 moles of ammonia at 25.0°C. 2. Calculate K for the decomposition of 2.00 moles of ammonia at NH3 is...
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