H2 at 1.75 atm and O2 at 0.75 atm are placed in a container at 200 degree C. A spark causes the reaction to form H2O (g). At equilibrium the total pressure is 1.90 atm. PLEASE SHOW WORK.
a. Calculate Kp (answer: 32)
b. Calculate Kc (answer: 1.2 x10^3)
Answer:-
the answer is given in the image,


H2 at 1.75 atm and O2 at 0.75 atm are placed in a container at 200...
13.52 g of H2 gas and 213.1 g of O2 gas are placed in a 413 mL rigid container. Calculate the equilibrium concentration of H2O yielded inside the container of 513 K if the Kc for this reaction is 313.
1. 2 SO3(g) ⇄ 2 SO2(g) + O2(g) Kp = 1.2× 10-5 0.60 atm of SO3 and 0.30 atm of SO2are placed in a container and the system is allowed to reach equilibrium. Calculate the pressure of O2(g) at equilibrium.? 2. Find the pH of 0.68 M HCOOH(aq) given that its Ka = 1.8×10-4. 2 questions please answer both
When 1.30 mol CO2 and 1.30 mol H2 are placed in a 3.00-L container at 395 ∘C, the following reaction occurs: CO2(g)+H2(g)⇌CO(g)+H2O(g). Part A: If Kc = 0.802, what are the concentrations of CO2 in the equilibrium mixture? Part B: If Kc = 0.802, what are the concentrations of H2 in the equilibrium mixture? Part C: If Kc = 0.802, what are the concentrations of CO in the equilibrium mixture? Part D: If Kc = 0.802, what are the concentrations...
5. A mixture of H2 gas (PH2 2.05 atm), CO2 gas (Pco2 4.10 atm) and water vapor (PH20-3.28 atm) are allowed to come to equilibriurm in a closed container. The temperature is 500. K. The equilibrium represented by the equation below is established and the equilibrium partial pressure of H20 is determined to be 3.51 atm. a) Find the equilibrium partial pressures of the CO2, H2, and CO gases. CO2 (g) H2 (g) ←→ CO (g) H2O (g) + +...
1- At a certain temperature, 0.820 mol of SO3 is placed in a 2.50-L container. 2SO3(g)---->2SO2(g)+O2(g) At equilibrium, 0.120 mol of O2 is present. Calculate Kc. 2- At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g)----->2HI(g) At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium? 3-Carbon disulfide is prepared by heating sulfur and charcoal....
A sample of solid NH4NO3 is placed in an
empty container. It decomposes according to the following
reaction:
NH4NO3(s) ⇔
N2O(g) + 2H2O(g)
At equilibrium, the total pressure in the container is 2.25 atm.
Calculate Kp.
1. 1.75 moles of H202 were placed in a 2.50 L reaction chamber at 307°C. After equilibrium was reached, 1.20 moles of H202 remained. Calculate the equilibrium constant, Kc, for the reaction. 2. Phosgene, COCl,, a poisonous gas, decomposes according to the equation COC2(g) CO(g)+ Cl2(g) Calculate Kp for this reaction if Kc- 0.083 at 900°C. K K.(PT) 3. Calculate Kc for the reaction 2HI(g) H2(g) +12(g) given that the concentrations of each species at equilibrium are as follows: [HI...
If 0.1500 mol of O2 (g) is placed in an empty 32.80-L
container and equilibrium is reached at 4000 K, one finds the
pressure is 2.175 atm. Find KP
and G for O2
(g) <--> 2 O (g) at 4000 K. Assume
ideal gases.
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One mole of N2 and 3 moles of H2 are placed in a flask at 397°C. Calculate the total pressure of the system at equilibrium if the mole fraction of NH3 is found to be 0.182. The KP for the reaction is 4.31 ×10−4. atm ** answer is not 12.364 atm
The elementary reaction 2H2O(g)−⇀↽−2H2(g)+O2(g)2H2O(g)↽−−⇀2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O,H2O, H2,H2, and O2O2 reach 0.0200 atm,0.0200 atm, 0.00550 atm,0.00550 atm, and 0.00700 atm,0.00700 atm, respectively. What is the value of the equilibrium constant at this temperature? kp= ?