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Chemistry
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At a certain temperature, 0.960 mol SO 3 placed in a 1.50 L container. 2 SO 3 (g) rightleftharpoons2SO 2 (g)+O 2 (g) At equilibrium, 0.190 mol O 2 is present. Calculate K c
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- Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 5.96 × 104: H₂(g) + Cl₂(g) →2 HCl(g) Use this information to complete the following table. Suppose a 46. L reaction vessel is filled with 1.8 mol of HCI. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 HCl(g) H₂(g) + Cl₂(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 H₂(g)+2Cl₂(g) 4 HCl(g) ܢܢ There will be very little H₂ and Cl₂. There will be very little HCI. Neither of the above is true. K = 0 K = 0 x10 X 0/3 ? olo 18 Ar BAarrow_forwardSuppose a 500. mL flask is filled with 1.7 mol of Cl₂, 1.1 mol of CHCl3 and 1.3 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHCl3 (g) → HC1(g) +CC14 (g) The equilibrium constant K for this reaction is 9.41 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. 10999arrow_forwardSuppose a 500. mL flask is filled with 0.30 mol of Br₂, 1.2 mol of OC1, and 0.60 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂ (g) BrOCI(g) + BrCl(g) The equilibrium constant K for this reaction is 4.09 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.arrow_forward
- Suppose a 250. mL flask is filled with 0.70 mol of NO₂, 0.20 mol of NO and 1.9 mol of CO₂. The following reaction becomes possible: NO₂ (g) + CO (g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.715 at the temperature of the flask. Calculate the equilibrium molarity of NO₂. Round your answer to two decimal places.arrow_forwardSuppose a 250. mL flask is filled with 1.1 mol of Cl2, 0.20 mol of CHCl3 and 2.0 mol of HCl. The following reaction becomes possible: Cl2(g) + CHCl3(g) HCl(g) +CCI4(g) The equilibrium constant K for this reaction is 0.652 at the temperature of the flask. Calculate the equilibrium molarity of HCI. Round your answer to two decimal places. Ом X Garrow_forwardAt a certain temperature, the equilibrium constant K for the following reaction is ×2.0510−7 : Br2g + OCl2g BrOCl g+BrClg Use this information to answer the following question. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K= 3Br2 (g) +3OCl2 (g) 3BrOCl (g) +3BrCl (garrow_forward
- Keq from Equilibrium Composition, Variously Expressed. At some temperature, an equilibrium mixture, in a 1.00-L container, involving the chemical system PCI5(g) = PCI3(g) + Cl2(g) is found to contain 5.74x1020 molecules of PCI5, 0.00921 mol of PCI3, and 0.228 g of Cl2. Calculate the equilibrium constant (Keg expressed in terms of the molar concentrations) at this temperature. (No units required.)arrow_forwardEnter your answer in the provided box. The equilibrium constant K. for the equation 2H2(g) + CO(g)=CH3OH(g) is 13 at a certain temperature. If there are 2.21 × 102 moles of H2 and 2.33 x 103 moles of CH;OH at equilibrium in a 4.31-L flask, what is the concentration of CO? Marrow_forwardSuppose a 250. mL flask is filled with 1.4 mol of CO, 1.9 mol of H₂O and 1.0 mol of CO₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) 2 The equilibrium constant K for this reaction is 9.28 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X Ś ?arrow_forward
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