Question

In: Chemistry

Consider the following unbalanced equation at some constant temperature: CO2(g) ⇌ CO(g) + O2(g)     K = 9.7...

Consider the following unbalanced equation at some constant temperature: CO2(g) ⇌ CO(g) + O2(g)     K = 9.7 x 10-6 In an experiment, 5.5 mol of CO2 and 3.1 mol of CO are initially placed into a 1.0 L rigid container. Calculate the concentration of O2 when the reaction has reached equilibrium. Please use the correct number of significant figures when entering your answer and enter your answer using exponential format. For example 1.00 x 10-27 should be entered as 1.00E-27.

Solutions

Expert Solution


Related Solutions

Consider the following unbalanced equation at some constant temperature: CO2(g) ⇌ CO(g) + O2(g)     K = 9.7...
Consider the following unbalanced equation at some constant temperature: CO2(g) ⇌ CO(g) + O2(g)     K = 9.7 x 10-6 In an experiment, 5.5 mol of CO2 and 3.1 mol of CO are initially placed into a 1.0 L rigid container. Calculate the concentration of O2 when the reaction has reached equilibrium. Please use the correct number of significant figures when entering your answer and enter your answer using exponential format. For example 1.00 x 10-27 should be entered as 1.00E-27.
Consider the equilibrium N2(g) + O2(g) ⇄ 2 NO(g) At 2300 K the equilibrium constant K...
Consider the equilibrium N2(g) + O2(g) ⇄ 2 NO(g) At 2300 K the equilibrium constant K = 1.7 × 10-3. Suppose that 0.0150 mol NO(g), 0.250 mol N2(g), and 0.250 mol O2(g) are placed into a 10.0-L flask and heated to 2300 K. The system is not at equilibrium. Determine the direction the reaction must proceed to reach equilibrium and the final equilibrium concentrations of each species. to the right to the left [N2] =____ mol/L [O2] = ____mol/L [NO]...
Consider the combustion of butane: C4H10(g) +O2(g)->CO2(g)+H2O(l) (unbalanced) Let 2.00 g of butane gas and 3.05...
Consider the combustion of butane: C4H10(g) +O2(g)->CO2(g)+H2O(l) (unbalanced) Let 2.00 g of butane gas and 3.05 atm of oxygen gas completely react (limiting) in a 2.00-L container at 125C. 2.1 Will there be a net increase or decrease in total pressure after the reaction is complete? 2.2 After complete reaction, what will be the mole fraction of H2O gas in the system?
PART A.Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) 1.K=[NO][N2][O2] 2.K=[NO]2[N2][O2] 3.K=[N2][O2][NO]2...
PART A.Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) 1.K=[NO][N2][O2] 2.K=[NO]2[N2][O2] 3.K=[N2][O2][NO]2 4.K=2[NO][N2][O2] PART B. The equilibrium-constant of the reaction NO2(g)+NO3(g)⇌N2O5(g) is K=2.1×10−20. What can be said about this reaction? 1.At equilibrium the concentration of products and reactants is about the same. 2.At equilibrium the concentration of products is much greater than the concentration of reactants. 3.At equilibrium the concentration of reactants is much greater than that of products. 4.There are no reactants left over once...
The system CO2(g) + H2(g) H2O(g) + CO(g) is at equilibrium at some temperature. At equilibrium,...
The system CO2(g) + H2(g) H2O(g) + CO(g) is at equilibrium at some temperature. At equilibrium, a 4.00L vessel contains 1.00 mole CO2, 1.00 mole H2, 2.40 moles H2O, and 2.40 moles CO. How many moles of CO2 must be added to this system to bring the equilibrium CO concentration to 0.669 mol/L? A. 0.498 moles B. 0.993 moles C. 0.429 moles D. 0.069 moles
Consider the reaction: 2 CO2(g) + Heat = 2 CO(g) + O2(g) 1.  Predict the effect on...
Consider the reaction: 2 CO2(g) + Heat = 2 CO(g) + O2(g) 1.  Predict the effect on the equilibrium system if the reaction temperature is decreased. (You may wish to write the equilibrium constant expression for the reaction first). a) The equilibrium will shift to the right favoring the products. b) The equilibrium will shift to the side that the light side of the force is on. c) There will be no effect. d) The equilibrium will shift to the left...
Consider the following equilibrium: CO2(g) + H2(g)---CO(g) + H2O(g); Kc = 1.6 at 1260 K Suppose...
Consider the following equilibrium: CO2(g) + H2(g)---CO(g) + H2O(g); Kc = 1.6 at 1260 K Suppose 0.038 mol CO2 and 0.022 mol H2 are placed in a 1.50-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g)? The answer is either 9.9 atm or 1.1 atm. But my question is WHY IS ONE CHOICE INCORRECT since I get both in my calculations.
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) K=0.118 at 4000 K A reaction mixture initially contains a CO partial...
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) K=0.118 at 4000 K A reaction mixture initially contains a CO partial pressure of 1361 mbar and a H2O partial pressure of 1781 mbar at 4000 K. Part A: Calculate the equilibrium partial pressure of CO in bar using three decimal places Part B: Calculate the equilibrium partial pressure of H2O in bar using three decimal places. Part C: Calculate the equilibrium partial pressure of CO2 in bar using three decimal places Part D: Calculate the...
Use the following equation (unbalanced) to solve the following series of problems. Ca(s) + O2(g) -->CaO(s)...
Use the following equation (unbalanced) to solve the following series of problems. Ca(s) + O2(g) -->CaO(s) What mass of calcium will react with oxygen gas in a 10.500 L container at a pressure of 10.0 atm and 500.°C? If 25.7 g of calcium reacts with oxygen gas, how many L of oxygen gas will be consumed at STP? How many g of CaO can be made from 150.0 mL of oxygen gas at 140°C and 1.52 atm? If 1.5 kg...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1336 torr and a H2O partial pressure of 1764 torr at 2000 K. Part A Calculate the equilibrium partial pressure of CO2. Part B Calculate the equilibrium partial pressure of H2.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT