he minerals magnetite (Fe302) and hematite (Fe2O3) xygen. exist in equilibrium with atmospheric a. b. 4 Fe304 (s) + O2 (g) = 6 Fe2O3 (S) Kp = 2.5 x 1087 at 298 K Determine the partial pressure of oxygen at equilibrium for this reaction. The partial pressure of oxygen in air is 0.21 atm. In which direction proceed to get to equilibrium? c. At room temperature, both magnetite and hematite are stable long time. Using principles we have learned, why might this be so? will the reaction in air for a very, VERY

For the equilibrium N2(g)+O2 <-->2NO(g), Kp = 0.0017 at 2300 K. At a given point, the partial pressures of the gases are PN2=PO2 = 0.660 atm and PNO= 0.0272atm. Which statment below is true? a. Q < K, so the reaction will continue to make more products. b. Q > K, so the reaction will consume products to make more reactants. c. Q = K, so the system is at equilibrium. d. The value of K will decrease until it is equal to Q. Show your work:

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)

Carbon tetrachloride can be produced by the following reaction: CS₂(g) + 3 Cl₂ (g) S₂Cl₂(g) + CCL (g) Suppose 1.20 mol of CS₂ and 3.60 mol of Cl₂ were placed in a 1.00-L flask at an unknown temperature. After equilibrium has been achieved, the mixture contains 0.23 mol CCl4. Calculate Ke at the unknown temperature. Ke- Submit Answer Try Another Version References] 10 item attempts remaining

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Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas. PCl3(g) + Cl2(g)  PCl5(g). A gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is allowed to equilibriate at 450 K. At equilibrium the partial pressures of the three gases are PPCl3 = 0.128 atm, PCl2 = 0.141 atm, and PPCl5 = 1.21 atm. (a) What is the value of Kp at this temperature? ______ (b) Does the equilibrium favor reactants or products? The equilibrium favors products. The equilibrium favors reactants.     Neither reactants nor products are favored.

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3. Consider the reaction Br2 (g) + Cl2 (g) 2 BrCl (g) Kp = 1.11 x 104 at 150 K. A reaction mixture initially contains a Br2 partial pressure of 0.993 atm and a Cl2 partial pressure of 0.967 atm at 150 K. Calculate the equilibrium partial pressure of each reactant and product. 4. Consider the reaction CO₂ (g) + H2 (g) A reaction mixture initially contains a CO partial pressure of 1.768 atm and a H₂O partial pressure of 2.324 atm at 2000 K. Calculate the equilibrium partial pressures of each reactant and product. CO (g) + H₂O (g) Kp = 0.0611 at 2000K.

2. Use the following information to calculate Kp and Ke for each reaction at 1000 K. CO2(g) + C(s) = 2C0(g) Kp = 1.50 at 1000 K a. 2c0(g) = CcO2(g) + C(s) 1 b. ½ CO2(g) + ½ C(s) = CO(g) c. 4C0(g) = 2CO2(g) + 2C(s)

An empty steel container is filled with 3.10 atm of H₂ and 3.10 atm of F2. The system is allowed to reach equilibrium. If Kp = 0.450 for the reaction below, what is the equilibrium partial pressure of HF? H₂ (g) + F₂ (g) → 2 HF (g)