Iron(III) oxide and hydrogen react to form iron and water, like this: Fe,0,(0)+3 H,(0)-2 Fe(s)+3 H,O(0) At a certain temperature, a chemist finds that a 9.5 L reaction vessel containing a mixture of iron(I) oxide, hydrogen, iron, and water at equilibrium has the following composition: compound amount Pe,O, 241 H, 3.53 Fe 4.06 g H,0 1.72 Calculate the value of the equilibrium constant K, for this reaction, Round your answer to 2 significant digits. OP

Iron(III) oxide and hydrogen react to form iron and water, like this: Fe,O3(s)+3 H2(9)–→2 Fe(s)+3 H,O(g) At a certain temperature, a chemist finds that a 4.5 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has the following composition: compound amount Fe,O3 3.54 g H2 3.20 g Fe 4.49 g H,O 1.06 g Calculate the value of the equilibrium constant K_ for this reaction. Round your answer to 2 significant digits.

Fill in the missing reactant, reagent and products. Indicate stereochemistry if necessary. Unless otherwise specified, assume the reagents are in excess.

Titanium(IV) chloride decomposes to form titanium and chlorine, like this: TİCL,(1)→Ti(s)+2 Cl,(9) 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 Cl2 1.40 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = ] x10

When 7.121 x 10-1 mol of NH3 and 7.121 x 10-1 mol of O2 are introduced into a 2.305 L reaction vessel at a certain temperature a chemist finds that at equilibrium the N2 concentration is 1.003 x 10-1 M: 4NH3(g) + 3O2(g) <==> 2N2(g) + 6H2O (g) What is the value of Kc for this reaction ?

A student artificially pumped 1 mole of each substance seen below in a piston with a moveable lid (this lid can increase or decrease thereby changing the volume and pressure): 2 C3H7OH (g) + 902 (g) 6 CO2 (g) +8 H2O(g) If the student increased the volume of the piston, how will the reaction shift to reach a new equilibrium? No conclusion can be made since more information is needed The reaction will shift to the left The reaction will shift to the right The reaction will not shift because Q = K

Calculating an equilibrium constant from a partial equilibrium composition 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 a 500. mL flask with 3.3 atm of ammonia gas and 0.87 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.6 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 P ☐ x1 x10 ☑ 5

Consider the following reaction where Kc = 7.00 × 10-5 at 673 K. NH₂I(s) NH3(g) + HI(g) A reaction mixture was found to contain 0.0532 moles of NHI(s), 0.00571 moles of NH3(g), and 0.00837 moles of HI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction must run in the forward direction to reach equilibrium. © must run in the reverse direction to reach equilibrium. O is at equilibrium.

Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N2(9) + 2 H,O(g) 2 NO(g) + 2 H2(g) → Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, water, nitrogen monoxide, and hydrogen has the following composition: compound pressure at equilibrium N2 92.2 atm H,O 76.1 atm NO 19.3 atm H2 33.6 atm Calculate the value of the equilibrium constant K, 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 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