Titanium(IV) chloride decomposes to form titanium and chlorine, like this: TiCl(1)→Ti(s)+2Cl,(g) At a certain temperature, a chemist finds that a 3.4 L reaction vessel containing a mixture of titanium(IV) chloride, titanium, and chlorine at equilibrium has the following composition: compound amount TiCl, 3.86 g Ti 2.68 g Cl, 1.40 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.

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

3. Nitrogen gas and oxygen gas can combine to produce nitrogen monoxide. At 1500 K the equilibrium constant, Ke, is 1.0 x 10 . Suppose a sample of air has [N2] = 0.80 M and [O2] = 0.20 M before any reaction occurs. Calculate the equilibrium concentrations of product and reactants at equilibrium at this temperature.

At a certain temperature, the equilibrium constant K for the following reaction is 0.0087: NO₂(g) + CO(g) → NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 29. L reaction vessel is filled with 0.27 mol of NO₂ and 0.27 mol of CO. 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 2 significant digits. NO(g) + CO₂(g) NO₂(g) +CO(g) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO₂(g)+2CO(g) 2NO(g)+2CO₂(g) There will be very little NO₂ and Co. There will be very little NO and CO₂. Neither of the above is true. K = 0 0 0 x10 X ?

Mercury and oxygen react to form mercury (II) oxide, like this: 2 Hg() +O₂(g)-2 HgO(s) At a certain temperature, a chemist finds that a 8.5 L reaction vessel containing a mixture of mercury, oxygen, and mercury(11) oxide at equilibrium has the following composition: compound amount Hg 20.5 g 0₂ 12.5 g Hgo 17.3 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K-O Submit Assic

Coal can be used to generate hydrogen gas (a potential fuel) by the following endothemic reaction (heat is on the reactant side of the equation). C (3) + H20 (g) = co (g) + H2 (g) If this reaction mixture is at equilibrium, predict whether each of the following will resuit in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. Part A adding more C to the reaction mixture the formation of additional hydrogen gas the formation of less hydrogen gas O no effect on the quantity of hydrogen gas

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

Iron and water react to form iron (III) oxide and hydrogen, like this: 2 Fe(s) + 3 H₂O(g) →Fe₂O3(s)+3H₂(g) At a certain temperature, a chemist finds that a 2.7 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound amount Fe 3.39 g H₂O 2.88 g Fe₂O3 2.96 g H₂ 3.61 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K 0 X ?

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

Ammonia has been studied as an alternative " clean " fuel for internal combustion engines , since its reaction with oxygen produces only nitrogen and water vapor and in the liquid form it is easily transported . An industrial chemist studying this reaction fills is a 50.0 L tank with 4.2 mol of ammonia gas and 19. mol of oxygen gas , and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 1.9 mol Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture . Round your answer to 2 significant digits