Calcium oxide is used to remove the pollutant SO2 from smokestack gases. The overall reaction is: CaO(s)+SO2​(g)+1/2​O2​(g)-->CaSO4​(s) For this reaction, Kp = 2.38 × 1015. a. What is the partial pressure of SO2 in equilibrium with air and solid CaO if PO2 in air is 0.21 atm? b. Consider a sample of gas that contains 475  moles of smokestack gas. How many molecules of SO2 are contained in this sample?

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A flask is charged with 1.5 atm of N2O4 (g) and 1 atm NO2 (g) at 20°C and the following equilibrium is achieved: N204 (g) 2 NO2 (g). After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. a. What is the equilibrium partial pressure of N2O4 b. Calculate the value Kp for the reaction. c. Calculate Kc for the reaction.

In a particular experiment 1.0 mole of H2O (g) and 1.0 mole of CO (g) are put into a flask and heated to 350 oC.  In another experiment 1.0 mol of H2 (g) and 1.0 mole of CO2 (g) are put into a different flask with the same volume as the first.  This mixture is also heated to 350 oC.  After equilibrium is reached, will there be any difference in the composition of the mixture in the two flasks?

12. Consider the chemical reaction 2HCl(g) H2(g) + Cl2(g). It contains 8.0 mol HCI, 0.20 mol H₂ and 0.40 mol Cl₂ in a 1.00 L flask at equilibrium. Calculate Kc and Kp at 300. °C. for the reaction.

At 125°C, Kp = 0.25 for the reaction 2NaHCO3(s) Na2CO3 (s) + CO2 (g) + H2O(g) A 1.00-L flask containing 39.7 g NaHCO3 is evacuated and heated to 125°C. a. Calculate the partial pressures of CO2 and H2O after equilibrium is established. Partial pressure of CO2 = Partial pressure of H2O = atm atm b. Calculate the masses of NaHCO3 and Na2CO3 present at equilibrium. Mass of NaHCO3 = Mass of Na2CO3 g g c. Calculate the minimum container volume necessary for all of the NaHCO3 to decompose. Volume = L

6. Determine the equilibrium constant (Kp) for the following reaction at 25°C. a. 2H20 (l) —> 2H2 (g) + O2 (g) b. 2O3 (g) —> 3O2 (g) Thank you!

11. PLease refer to the attached photo. THank youuu

The two most abundant atmospheric gases react to a small extent at 298K as shown below: N2 (g) + O2 (g) → 2NO (g) Kp = 4.35x10-31 a. What are the equilibrium pressures of each species when 0.210atm of N2 and 0.780atm of O2 are introduced into a 1.00L container? b. What is the value of Kc at 298K? Kp = Kc(RT)An R = 0.0821 c. What are the equilibrium concentrations of each species if the initial concentration of N2 is 0.100M and the initial concentration of O2 is 0.100M?

2. Use the following information to calculate Kp and Ke for each reaction at 1000 K. CO2(g) + C(s) = 2C0(g) Kp = 1.50 at 1000 K a. 2c0(g) = CcO2(g) + C(s) 1 b. ½ CO2(g) + ½ C(s) = CO(g) c. 4C0(g) = 2CO2(g) + 2C(s)