14. An industrial chemist introduces 1.1 atm H2 and 1.1 atm CO2 into a 1.00-L container...
An industrial chemist introduces 3.3 atm H2 and 3.3 atm CO2 into a 1.00-L container at 25.0°C and then raises the temperature to 700.0°C, at which Keq = 0.534: H2(g) + CO2(g) ⇔ H2O(g) + CO(g) How many grams of H2 are present after equilibrium is established? Please present work and solution
An industrial chemist puts 1.25 mol each of H2(g) and CO2(g) in a 1.00-L container at a certain temperature. When equilibrium is reached, 0.56 mol of CO(g) is in the container. Find Keq at this temperature for the following reaction: H2(g) + CO2(g)↔H2O(g) + CO(g)
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) + +...
For the reaction system: H2 (g) + CO2 (g) → H2O (g) + CO (g) The equilibrium constant is 1.60 at a certain temperature. 1.00 mole each of hydrogen, carbon dioxide is placed in a sealed 5.00 L container. After equilibrium is established, determine the molarity (M) of each species.
16. Enter your answer in the provided box. For the reaction H2(g) + CO2(g) ⇆ H2O(g) + CO(g) at 700°C, Kc = 0.534. Calculate the number of moles of H2 that are present at equilibrium if a mixture of 0.720 mole of CO and 0.720 mole of H2O is heated to 700°C in a 50.0−L container. _______ mol
9. The first step in industrial nitric acid production is the catalyzed oxidation of ammonia. Without a catalyst, a different reaction predominates: 4NH3(g) +302(g) 2N2( ) + 6H 20(g) When 0.0260 mol gaseous NHs and 0.0240 mol gaseous O-, are placed in a 1.00 L container at a certain temperature, the Ns concentration at equilibrium is 2.80x 10 3 M. Calculate Keg for the reaction at this temperature. Submit Answer Tries 0/99
11. When 0.941 mol of gaseous HI is sealed in a 1.00-L flask at 225°C, it decomposes until the equilibrium amount of 12 present is 0.171 mol: 2HI() H2(9)+ I2(9) Use these data to calculate Keg for this reaction at 225°C. Submit Answer Tries 0/99
An equilibrium mixture was found to have the following composition in a 1.00 L flask: H2 CO2 H2O CO 0.630 0.590 0.210 0.280 moles What is the equilibrium constant for the following gas phase reaction? H2 + CO2 H2O + CO K = How many moles of H2O must be removed in order to increase the number of moles of CO at equilibrium to 0.553 mol? mol H2O -/12 points v An equilibrium mixture was found to have the following...
2. 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 system. The following equilibrium is established at 500 K CO2(g) + H2(c) -> CO(S) + H2O(g) At equilibrium, Prao = 3.51 atm. A) Calculate the equilibrium partial pressures of CO2. Hz, and CO (6 points) and B) Calculate Kfor the reaction (4 points). Recall PV = nRT, with R = 0.0821 L-atm/mol-K. Hint: ICE chart not necessary. Notice...
Imagine a 1.00 L container which initially contains 0.250 atm of H2O and CO each construct and complete an ICE table and determine the equilibrium concentrations of each gas