Phosphorus tribromide decomposes to form phosphorus and bromine, like this: 4 PBr3(g) → P4(g) + 6 Br,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of phosphorus tribromide, phosphorus, and bromine has the following composition: compound concentration at equilibrium PBR3 1.8M P4 1.3 M Br2 1.7M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0

Equilibrium constant, Kc, for the following reaction is 8.08×10-3 at 1080 K.2SO3(g) 2SO2(g) + O2(g)Calculate the concentration of SO3 in the equilibrium mixture?When a sufficiently large sample of SO3(g) is introduced into an evacuated vessel at 1080 K, the equilibrium concentration of O2(g) is found to be 9.70×10-2 M.

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N₂(g) + 3 H₂(g) ⇒ 2 NH3 (g) K₂=8.x 10-7 He fills a reaction vessel at this temperature with 5.0 atm of nitrogen gas and 6.8 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NH3 at right. Round your answer to 1 significant digit. Oyes O no atm 10 X

Phosphorus tribromide decomposes to form phosphorus and bromine, like this: 4 PB13(g) → PĄ(9) + 6 Br,(9) Also, a chemist finds that at a certain temperature the equilibrium mixture of phosphorus tribromide, phosphorus, and bromine has the following composition: compound concentration at equilibrium PB13 0.66M BA 0.79M Br2 0.62M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = ] x10

Hydrogen chloride and oxygen react to form chlorine and water, like this: 4 HCl(g) + O,(g) 2 Cl,(g) + 2 H,0(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, oxygen, chlorine, and water has the following composition: compound concentration at equilibrium HCl 0.46 M O2 1.1M Cl2 1.2 M H20 0.21 M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0 Check Explanation O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy | Accessibility

Calcium oxide and carbon dioxide react to form calcium carbonate, like this: CaO(s)+CO2(g)→CaCO3(s) At a certain temperature, a chemist finds that a 4.4 L reaction vessel containing a mixture of calcium oxide, carbon dioxide, and calcium carbonate at equilibrium has the following composition: compound amount Cao 31.2 g CO2 16.8 g CACO3 32.3 g Calculate the value of the equilibrium constant K̟ for this reaction. Round your answer to 2 significant digits. K = [| Submit A Continue MacBook Air F10

Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)→2 HgO(5) At a certain temperature, a chemist finds that a 3.6 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 9.7 g O2 21.8 g HgO 10.2 g Calculate the value of the equilibrium constant K̟ for this reaction. Round your answer to 2 significant digits. K_ = 0

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N2(g) + 2H2O(g) 2 NO(g) + 2 H2(g) K=2.x 10 -10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 11. atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H2, using only the tools available to you within ALEKS? ○ yes x10 O no If you said yes, then enter the equilibrium pressure of H₂ at right. Round your answer to 1 significant digit. atm 5

At a certain temperature, the equilibrium constant K for the following reaction is 3.1 × 10 : H,(g) + I,(g) = 2 HI(g) Use this information to complete the following table. Suppose a 36. L reaction vessel is filled with 1.7 mol of HI. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little H2 and I2. There will be very little HI. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = 1 2 HI(g) H2(9)+I,(9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = I 2 H,(9)+21½(9) 4 HI(g)

Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(9)→2 HgO(s) At a certain temperature, a chemist finds that a 10. L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 12.7 g O2 13.4 g HgO 15.5 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = | Submit Assignm Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center| Access 43.203 FEB 19 MacBook Air