CO2 (g) is placed in a sealed 5.0L vessel at 701 K and 10.0 atm. The vessel is heated to 1401K and the CO2 (g) partially decomposes to CO )g) and O2 (g). The final pressure in the vessel is 22.5 atm.
a. What is the complete balanced equation for this reaction?
b. How many moles of CO2 are present in the vessel initially (show work)
c. How many moles are present in the flask at the end of the reaction?
d. How many moles of CO2 CO and O2 are present in the flask after the reaction?
e. What is the partial pressures due to CO2, CO, and O2 in the flask at the end of the reaction?
CO2 (g) is placed in a sealed 5.0L vessel at 701 K and 10.0 atm. The...
A mixture of 0. 166 moles of C is reacted with 0.117 moles of O2 in a sealed, 10.0 L vessel at 500.0 K, producing a mixture of CO and CO2 3C(s)+2O2(g) → 2CO(g) + CO2(g) The total pressure is 0.707 atm. What is the partial pressure of CO?
how to solve this?
Sulphur trioxide decomposes at high temperature in a sealed container: 2 SO3(g) <--> 2 SO2(g) + O2(g). Initially, the vessel is charged at 1000 K with SO3(g) at a partial pressure of 0.500 atm. At equilibrium the SO3 partial pressure is 0.200 atm. Calculate the value of Kp at 1000 K to 3 decimal places.
A mixture of0.147 moles of C is reacted with 0.117 moles of O2 in a sealed, 10.0 L-vessel at 500.0 K, producing a mixture of CO and CO2. The limiting reagent of the below reaction is carbon. For0.147 moles of carbon, determine the amounts of products (both the CO and CO2) formed in this reaction. Also, determine the amount of O2 remaining and the mole fraction of CO when the reaction is complete. How many mol CO2 formed? How many...
A mixture of 0.156 moles of C is reacted with 0.117 moles of O2 in a sealed, 10.0 L vessel at 500.0 K, producing a mixture of CO and CO2. 3C(s)+2O2(g)---> 2CO(g)+CO2(g) The total pressure is 0.693 atm. What is the partial pressure of CO? atm
A sealed reaction vessel initially contains 1.632x102 moles of water vapor and 1.113x102moles of COlg H2O(g) +Co(g)H2(g) +CO2(g After the above reaction has come to equilibrium, the vessel contains 8.326x10-3 moles of CO2lg) 4th attempt hi See Periodic Table See Hint Feedback What is the value of the equilibrium constant Kcof the reaction at the temperature of the vessel? 2.487186887
A 10.0 g sample of NH4Cl(s) is heated in an initially evacuated 5.00 L flask to 900 C. The solid ammonium chloride dissociates into NH3(g) and HCl(g) as products; reaction has Kp= 1.44 at this temperature. A). Calculate the partial pressures of NH3(g) and HCl(g) present at equilibrium. B). Calculate the number of moles of NH3(g) and HCl(g) that will be present in the flask at equilibrium. You may neglect the volume of the solid and assume V=5.00 L.
A reaction vessel contains 13.1 g of CO and 13.1g of CO2. How many grams of CO2 could be produced according to the following unbalanced reaction? CO+O2→CO2
CaCO3(s) = Cao (s)+CO2 (g) When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxide gas, as represented by the equation above. A 2.0 mol sample of CaCO3(s) is placed in a rigid 100. L reaction vessel from which all the air has been evacuated. The vessel is heated to 898°C at which time the pressure of CO2(g) in the vessel is constant at 1.00 atm, while some CaCO3(s) remains in the vessel. a. Calculate...
1. A key step in the extraction of iron from its ore is FeO(s) + CO(g) ⇌ Fe(s) + CO2(g) Kp = 0.403 at 1,000°C This step occurs in the 700°C to 1,200°C zone within a blast furnace. What are the equilibrium partial pressures of CO(g) and CO2(g) when 1.1000 atm of CO(g) and excess FeO(s) react in a sealed container at 1000°C? 2. Compound A decomposes according to the equation A(g) ⇌ 2 B(g) + C (g) A...
At a particular temperature, K = 5.7 ✕ 10−6
for the following reaction.
2 CO2(g) 2
CO(g) + O2(g)
If 2.9 moles of CO2 is initially placed into a 4.6-L
vessel, calculate the equilibrium concentrations of all
species.