10 mol NH3(g) was placed in a previously evacuated 20-L container. After a sudden temperature rise...
10 mol NH3(g) was placed in a previously evacuated 20-L container. After a sudden temperature rise to 961.4K, 80% of ammonia dissociated into hydrogen and nitrogen according to the reaction:
2/3 NH3(g) ------> 1/3 N2(g) + H2(g)
What is the total pressure of the mixture, if all gasses are ideal? (correct sig-figs)
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10 mol NH3(g) was placed in a previously evacuated
20-L container. After a sudden temperature rise...
Ammonia, NH3(g)NH3(g), at a pressure of 1.13 bar, is placed in a container at a certain...
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
Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3 H2(g) + N2(g)...
Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3 H2(g) + N2(g) → 2 NH3(g). The value of AH is -92.38 kJ/mol, and that of AS is -198.2 J/mol · K. Determine AG at 50.00°C for the preparation of 2 moles of NH3. (answer in kJ/mol) Answer: -56.723 Check
A mixture of 0.02138 mol of C2H6, 0.006096 mol of N2, 0.01567 mol of NH3, and 0.02233 mol of C2H4 is placed in a 1.0-L s...
A mixture of 0.02138 mol of C2H6,
0.006096 mol of N2, 0.01567 mol of NH3, and
0.02233 mol of C2H4 is placed in a 1.0-L
steel pressure vessel at 5155 K. The following equilibrium is
established:
3 C2H6(g) + 1 N2(g)
2 NH3(g) + 3
C2H4(g)
At equilibrium 0.0006616 mol of N2 is found in
the reaction mixture.
(a) Calculate the equilibrium partial pressures of
C2H6, N2, NH3, and
C2H4.
Peq(C2H6) = .
Peq(N2) = .
Peq(NH3) = .
Peq(C2H4)...
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A 0.030-m^3 container is initially evacuated. Then, 4.0 g of water is placed in the container, and, after some time, all the water evaporates. If the temperature of the water vapor is 388 K, what is its pressure?
A mixture of 2.0 mol of H2(g) and 1.0 mol of O2(g) is placed in a...
A mixture of 2.0 mol of H2(g) and 1.0 mol of O2(g) is placed in a sealed evacuated container made of a perfect insulating material at 24 ∘C. The mixture is ignited with a spark and it reacts to form liquid water. (The specific heat for water vapor is 2.04 J/g⋅oC, and ∆Hvap = 44.0 kJ/mol) The heat generates in the exothermic reaction will heat the liquid water to boiling, vaporize it, and heat the vapor to its final temperature....
Question 10 of 23 > At a certain temperature, 0.4011 mol of N2 and 1.641 mol...
Question 10 of 23 > At a certain temperature, 0.4011 mol of N2 and 1.641 mol of H2 are placed in a 4.00 L container N2(g)+3 H2 g) 2NH3(g) At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, Ke
4. The equilibrium constant for the reaction is 2.60 x 10-7 at 300 °C. 2 NO2(g)...
4. The equilibrium constant for the reaction is 2.60 x 10-7 at 300 °C. 2 NO2(g) = 2 02(g) + N2(g) If 0.250 mol of NO, gas is placed in 5.00 L vessel and allowed to reach equilibrium at this temperature, calculate the equilibrium concentrations of the nitrogen gas and oxygen gas. (Ignoring X Method) s. For the following reaction: 2 NH3(g) = 3 H2(g) + N2(g) When 1.2 mol of hydrogen gas and 0.40 mol of nitrogen gas are...
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,...
N2(g) + 3 H2(g) ⇌ 2 NH3(g) KP = 6.78 x 105 at 298 K (determined...
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...
1. At a certain temperature, 0.338 mol CH4 and 0.808 mol H2O is placed in a...
1. At a certain temperature, 0.338 mol CH4 and 0.808 mol H2O is placed in a 4.00 L container. CH4(g)+2H2O(g)????CO2(g)+4H2(g) At equilibrium, 4.89 g CO2 is present. Calculate Kc. 2. At a certain temperature, 0.352 mol CH4 and 0.862 mol H2S are placed in a 1.50 L container. CH4(g)+2H2S(g)????CS2(g)+4H2(g) At equilibrium, 14.5 g CS2 is present. Calculate Kc . 3. At a certain temperature, 0.3211 mol of N2 and 1.501 mol of H2 are placed in a 2.50 L container....
Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3 H2(g) + N2(g) → 2 NH3(g). The value of AH is -92.38 kJ/mol, and that of AS is -198.2 J/mol · K. Determine AG at 50.00°C for the preparation of 2 moles of NH3. (answer in kJ/mol) Answer: -56.723 Check
A mixture of 0.02138 mol of C2H6,
0.006096 mol of N2, 0.01567 mol of NH3, and
0.02233 mol of C2H4 is placed in a 1.0-L
steel pressure vessel at 5155 K. The following equilibrium is
established:
3 C2H6(g) + 1 N2(g)
2 NH3(g) + 3
C2H4(g)
At equilibrium 0.0006616 mol of N2 is found in
the reaction mixture.
(a) Calculate the equilibrium partial pressures of
C2H6, N2, NH3, and
C2H4.
Peq(C2H6) = .
Peq(N2) = .
Peq(NH3) = .
Peq(C2H4)...
Question 10 of 23 > At a certain temperature, 0.4011 mol of N2 and 1.641 mol of H2 are placed in a 4.00 L container N2(g)+3 H2 g) 2NH3(g) At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, Ke
4. The equilibrium constant for the reaction is 2.60 x 10-7 at 300 °C. 2 NO2(g) = 2 02(g) + N2(g) If 0.250 mol of NO, gas is placed in 5.00 L vessel and allowed to reach equilibrium at this temperature, calculate the equilibrium concentrations of the nitrogen gas and oxygen gas. (Ignoring X Method) s. For the following reaction: 2 NH3(g) = 3 H2(g) + N2(g) When 1.2 mol of hydrogen gas and 0.40 mol of nitrogen gas are...
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