An equilibrium mixture of H2,I2 ,and HI at 458 °C contains 0.112 mol H2,0.112 mol I2,and 0.775 mol HI in a 5.00-L vessel
An equilibrium mixture of H2, I2, and HI at 458 ∘C contains 0.112 molH2, 0.112 molI2, and 0.775 molHI in a 5.00-L vessel. Part A: What are the equilibrium partial pressure of HI when equilibrium is reestablished following the addition of 0.200 mol of HI? Express your answer to four significant figures and include the appropriate units. Part B:What are the equilibrium partial pressure of I2 when equilibrium is reestablished following the addition of 0.200 mol of HI? Express your...
An equilibrium mixture contains 0.950 mol HI, 0.490 mol I2, and 0.290 mol H2 in a 1.00-L flask. What is the equilibrium constant for the following reaction? 2HI(g) H2(g) + I2(g) K = How many moles of I2 must be removed in order to double the number of moles of H2 at equilibrium? mol I2
A mixture of 0.01341 mol of CH4, 0.01170 mol of H2S, 0.02118 mol of CS2, and 0.02835 mol of H2 is placed in a 1.0-L steel pressure vessel at 3416 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g) 1 CS2(g) + 4 H2(g) At equilibrium 0.003198 mol of H2S is found in the reaction mixture. - Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2. - Calculate KP for this reaction.
25. A mixture of 0.100 mol of NO, 0.0500 mol of H2, and 0.100 mol of H2O is placed in a 1.00-L vessel. The following equilibrium is established: 2NO(g) + 2H2 (g) → N2(g) + 2H2O(g) At equilibrium [NO] -0.0620 M. Calculate the equilibrium concentrations of H2, N2, and H20.
When HI(g) is heated to 700 K, it reversibly decomposes to H2(g) and I2(g). The reaction is- 2 HI(g) ⇌ H2(g) + I2(g). A 15.00-L vessel at 700 K initially contains HI(g) at a pressure of 4.00 atm. When equilibrium is reached, it is found that the partial pressure of H2(g) is 0.387 atm. What is the partial pressure of HI(g) at equilibrium? A) 4.00 atm B) 3.61 atm C) 3.23 atm D) 4.39 atm E) 0.387 atm
At 6 oC the equilibrium constant for the reaction: 2 HI(g) H2(g) + I2(g) is KP = 2.66e-11. If the initial pressure of HI is 0.00837 atm, what are the equilibrium partial pressures of HI, H2, and I2? We were unable to transcribe this imageAt 6 °C the equilibrium constant for the reaction: 2 HI(g) = H2(g) + 12(g) is Kp = 2.66e-11. If the initial pressure of HI is 0.00837 atm, what are the equilibrium partial pressures of HI,...
7) a 1.50L glass vessel contains 0.112 mole of Cl2(g) and 0.117 mile of HI(g) at 210°C. A) starting with the ideal gas law, PV=nRT, solve for P/RT. What are the units for P/RT when simplified? B) calculate the molarities of the gases and convert those values into pressure using the ideal gas law. C) assume moles, temperature, and pressure stated above, if the following reaction goes to completion, what is the total pressure in the container? Assume constant temperature...
A gas mixture contains 0.600 mol of N2, 0.150 mol of H2, and 0.400 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 8.00 L vessel at 27.00°C. A) What is the total pressure in the vessel (atm)? B) What is the pressure (atm) of H2? C) What is the pressure (atm) of N2? D) What is the pressure (atm) of CH4?
A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium is established at 500 K: CO2(g)+H2(g)⇌CO(g)+H2O(g) Calculate the initial partial pressure of CO2. Calculate the initial partial pressure of H2. Calculate the initial partial pressure of H2O, H2 and CO2
A vessel of volume 22.4 dm3 contains 2.0 mol H2 and 1.0 mol N2 at 273.15 K initially. All the H2 reacted with sufficient N2 to form NH3. Calculate the partial pressures and the total pressure of the final mixture.