Mercury(II) oxide decomposes to form mercury and oxygen, like this: 2 HgO(s)→2 Hg(1) + O₂(g) At a certain temperature, a chemist finds that a 7.5 L reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has the following composition: compound amount HgO 20.7 g Hg 7.7 g 0₂ 10.5 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. =0 K = x10 X

Write the equilibrium constant expression. Solid carbon and carbon dioxide gas react and form carbon monoxide: C(s) + CO₂(g) = 2CO(g)

Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s)+3 H,0(g)→ Fe,O3(s)+3 H,(g) At a certain temperature, a chemist finds that a 9.2 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound amount ol. Fe 4.85 g Ar H,O 1.44 g Fe,O3 2.98 g H2 2.51 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 Ox10 Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

4 Titanium(IV) chloride decomposes to form titanium and chlorine, like this: Ticl,()-Ti(s)+2 Cl,(9) At a certain temperature, a chemist finds that a 7.7 L reaction vessel containing a mixture of titanium(IV) chloride, titanium, and chlorine at equilibrium has the following composition: compound amount TiCl, 4.90 g Ti 1.24 g Cl, 2.16 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0 Submit Assignment Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility Finder F12 F11 F9 F10 F8 F7 F5 F6 .

Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)–→2 HgO(s) At a certain temperature, a chemist finds that a 6.3 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 5.8 g O2 22.5 g HgO 18.9 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0

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

Carbon disulfide and chlorine react according to the following equation: CS2(g) + 3Ch(g) =S,Cl½(g) + CC1,(g) When 1.14 mol of CS, and 4.80 mol of Clh are placed in a 2.00-L container and allowed to come to equilibrium, the mixture is found to contain 0.650 mol of CC14. How many moles of Cl are present at on equilibrium? Select one: O a. 0.490 mol O b. 2.85 mol O c. 3.50 mol O d. 0.650 mol O e. 1.43 mol e to search F3 F4 F5 F6 FZ FB F9 F10 F11 F12 Prise %24 E R T G H K B N M 立

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

please see attached image

Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s) + 3 H₂O(g) → Fe₂O3(s)+ 3 H₂(g) At a certain temperature, a chemist finds that a 2.5 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound Fe H₂O Fe₂O3 H₂ amount 4.04 g 2.87 g 3.49 g 2.08 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. C K = 0 C Dx1 x10 X Ś