For each of the following reactions, indicate if the equilibrium mixture contains mostly products, mostly reactants, or both reactants and products:
a.
b.
c.
d.
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Basic Chemistry
- The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.arrow_forwardMustard gas, used in chemical warfare in World War I, has been found to be an effective agent in the chemotherapy of Hodgkin's disease. It can be produced according to the following reaction: SCl2(g)+2C2H4(g)S(CH2CH2Cl)2(g)An evacuated 5.0-1- flask at 20.0C is filled with 0.258 mol SCl2 and 0.592 mol C2H4. After equilibrium is established, 0.0349 mol mustard gas is present. (a) What is the partial pressure of each gas at equilibrium? (b) What is K at 20.0C?arrow_forward. Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose the system is already at equilibrium, and then an additional mole of CO2(g) is injected into the system at constant temperature. Does the amount of O2(g) in the system increase or decrease? Does the value of K for the reaction change?arrow_forward
- Consider the following system at equilibrium where AHⓇ 2SO2(g) + O2(g) = 2SO3 (9) When 0.24 moles of O₂ (g) are added to the equilibrium system at constant temperature: The value of K O increases decreases O remains the same The value of Qc O is greater than Kc O is equal to Kc O is less than Kc = 198 kJ, and Ke The concentration of SO2 will O increase decrease O remain the same The reaction must O run in the forward direction to reestablish equilibrium O run in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium = 34.5, at 1150 K: Consider the following mat equilibrium where&ff-879 PC)+)-PC, ( Whe036PC (a) are added to the equum system at The K The Q Ogra Therearrow_forwardNitrogen dioxide dimerizes according to the following reaction: 2 NO₂ (9) K₂ = 6.7 at 298 K N₂O4 (9) A 2.25-L container contains 0.055 mol of NO₂ and 0.082 mol of N₂O4 at 298 K. Part A Is the reaction at equilibrium? If not, in what direction will the reaction proceed? The reaction is at equilibrium. The reaction is not at equilibrium and will shift to the left. The reaction is not at equilibrium and will shift to the right.arrow_forwardGiven the following: (1) N₂O(g) + O2(g) = 2 NO(g) (2) N₂(g) + ½ O₂(g) = N₂O(g) A. 7.1×104 B. 2.9×10-26 Find the value of the equilibrium constant Kc for the following equilibrium reaction: N₂(g) + O₂(g) = 2 NO(g) C. 1.4×10-5 D. 2.6×10-22 Kc 1.7x10-13 M0.5 = E. 4.1×10-31 Кс = 2.4×10-18 M-0.5arrow_forward
- 9:10 Consider the equilibrium system described by the chemical reaction below. If 0.1908 moles of CO2, 0.0908 moles of H₂, 0.0092 moles of CO, and 0.0092 moles of H₂O are present in a 2.00 L reaction vessel at equilibrium at 300 K, what is the value of Kc of the reaction at this temperature? Question 5 of 10 CO₂(g) + H₂(g) = CO(g) + H₂O(g) 1 Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. Kc = Once the expression is constructed, solve for Kc. [0.1908] [0.0092] [0.0908]² [0.0092]² 1.1 Submit [0.0908] [0.0184] [2.00] [0.0184]² = [0.0954] [0.0046] [300] 200 Tap here or pull up for additional resources RESET [0.0454] [0.1908]² [0.0954]² 4.9 × 10-³arrow_forwardWill the equilibrium be established when following compounds are kept in a closed container and allowed time for equilibrium? (5)CaCO3(s) = CaO(s) + CO2(g)(a) CaCO3(s)(b) CaO(s) and CO2(g) at a pressure greater than the value of Kp(c) CaCO3(s) and CO2(g) at a pressure greater than the value of Kp(d) CaCO3(s) and CaO(s)(e) CaO(s) and CO2(g) at a pressure smaller than the value of Kparrow_forward9 Methanol is produced synthetically: CO (g) + 2H2 (g) CH;OH (g) A H=+24 Kcal a) Write the Equilibrium Constant Expression: b) Is it an Endothermic or Exothermic Reaction? c). Indicate the effect on the equilibrium, ie., does the reaction shift to the right, to the left, or have no effect on the reaction at all: 1. Increase in [2H2] = 2. Decrease in [CO] = 3. Increase in Temperature = 4. Increasc in Pressure = 5. Addition of a catalyst =,arrow_forward
- Iron(III) oxide and hydrogen react to form iron and water, like this: Fe,O3(s)+3 H,(g)-2 Fe(s)+3 H,0(9) At a certain temperature, a chemist finds that a 2.7 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has the following composition: compound amount Fe,O3 3.66 g H2 4.09 g Fe 4.46 g H2O 1.82 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy I Accessibility 29 MacBook Air D00 吕口 F3 F10 D00 F4 F5 F7 F8 F2 23 & 4 5 7 8 9 E R T Y | K L LLarrow_forwardAt a certain temperature, Kc = 0.18 for the following reaction:PCl3 (g) + Cl2 (g) PCl5 (g)Suppose a reaction vessel at this temperature contained these three gases at the following concentrations:[PCl3] = 0.420 M, [Cl2] = 0.240 M, [PCl5] = 0.00500 M:(10a): Is the system in a state of equilibrium? Justify your answer with a calculation.(10b): If the system is not in equilibrium, which direction will the reaction proceed to reach equilibrium?arrow_forward(12a) The equilibrium constant, Kp, for the following reaction is 0.636 at 600K. COCl2(g) CO(g) + Cl2(g)If an equilibrium mixture of the three gases in a 19.1 L container at 600K contains COCl2 at a pressure of 0.539 atm and CO at a pressure of 0.606 atm, the equilibrium partial pressure of Cl2 is _____ atm. (b) Consider the following reaction:COCl2(g) CO(g) + Cl2(g) If 4.06×10-2 moles of COCl2, 0.269 moles of CO, and 0.280 moles of Cl2 are at equilibrium in a 10.8 L container at 686 K, the value of the equilibrium constant, Kp, is ________arrow_forward
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