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According to Le Châtelier's principle, does the equilibrium shift in the direction of products or reactants when
a.
b.
c.
d.
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Basic Chemistry
- 4:15 Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into a 1.25 L flask at 25.0 °C. The flask is found to contain 2.35 g of NO2, 9.60 g of N₂O, and 4.50 g of O₂. What is the value of Kc for this reaction? 4 NO₂(g) 2 N₂O(g) + 3 O₂(g) Question 8 of 10 Kc = Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. [0.0409]² [0.218] [0.113] ³ [0.0409]¹ 0.480 Once the expression is constructed, solve for Kc. 3.57 x 10³ 1 [0.175]² [0.141] [0.0409] [0.175]4 0.0642 Submit [0.113]² [0.0409]³ [0.175] [0.113]4 28.7 Tap here or pull up for additional resources RESET [0.0511] [0.175]³ [0.113] 15.8 13.6arrow_forward13. 1. Using Le Chatelier’s principles, for the following equilibrium predict the direction that the equilibrium will shift, towards the products, towards the reactants or would it have no effect and go to neither. Mg(s) + 2HCl (aq) ⟷⟷ MgCl2 (aq) + H2 (g) ∆H = - 43 kcal/mole i. Decrease in Mg: Products Reactants Neither ii. Decrease in pressure: Products Reactants Neither iii. Increase in H2 : Products Reactants Neither iv. Increase in temperature: Products Reactants Neitherarrow_forwardIf at 400°C the equilibrium constant for the reaction NO2(g) + H2(g) = NO(g) + H₂O(g) has Kp = 7.28 x 10-6, what is AG for this reaction at 400°C? (1) 66.2 kJ/mol O (3) 654 kJ/mol O (4) 388 kJ/mol O (2) 39.3 kJ/mol # 3 A Moving to the next question prevents changes to this answer. E $ 4 R % 5 T C 6 MacBook Pro Y & 7 U * 8 - 9 K 0 0 L P Question 2 of + 11arrow_forward
- Given the following equilibrium system: 2SO2(g) + O2(g) ↔ 2SO3(g) + 99.1 kJ The pressure on the system is increased while the temperature is kept constant. Compared to its original concentration, how will the concentration of SO2(g) change? 1.) Decrease 2.) Increase 3.) Remain the Samearrow_forwardConsider the following system at equilibrium: P4 (g) + 6 H2 (g) = 4 PH3 (g) ΔΗ 110. 5 kJ If the volume was increased, what changes would have to occur to reestablish equilibrium? Select 2 correct answer(s) The reaction would shift right. The concentration of PH3 would increase. The concentration of P4 would increase The reaction would shift left. The concentration of H2 would decrease.arrow_forward10. 1) Please choose the corect expression and circle it. Le chatelier's Principle Summarized Below Change Concentration Pressure Volume Shifts Equilibrium Change Equilibrium Constant yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no yes/no Temperature Catalyst ii) 250:(g)+0:(3)2SO:(g) The position of equilibrium moves to the right/left if the concentration of SO; is increased. Co.(g) CO(g)+O( If we increase the pressure of COg), the system will shift towards the reactants/products because it has a fewer/more number of moles of gas. CIHH:0 HO'+Cl+Heat If we decrease the temperature, the reaction will proceed towards the reactants/products because the system must regenerate/used the heat that was lost/gain. iii) Will the equilibrium in reactionarrow_forward
- .50 mol of I2 and .50 mol of Br2 are placed in a 1.00 flask and allowed to reach equilibrium. At equilibrium, the flask contains .84 mol of IBr. What is the value of the Kc for this reaction? I2(g) + Br2(g) ---> 2 IBr(g) Group of answer choices 110 4.0 11 40.arrow_forward7. 2CO2 (g) 200(g) + O2 (g). It was found that at 20 OC, the total pressure at equilibrium is 2.9 atm and that of CO2 is 0.8 atm. Calculate K. (Answer 2.14)arrow_forwardIn (6.7 At 600 °C, what is the value of the equilibrium constant for: C (s) + 2 PCI5 (g) = 2 PC|3 (g) + CCl4 (1) ? a. 1.3x10-⁹ b. 2.4x10-4 d. 1.9x105 c. 5.3x104 12. At 600 °C, the following reactions have these equilibrium constants: PC15 = PC|3 (g) + Cl2 (g) K = 6.77 x 10-5 (g) C(s) + 2 C/₂ (g) = CCl4 (1) K = 5.31 x 10+4 MOMOarrow_forward
- Flag question Hydrogen peroxide decomposes according to the following reaction: 2H₂O2(g) — 2H₂O(g) + O2(9) In a particular experiment, 3.5 moles of H₂O2 were placed in a 2.0 L reaction chamber at 307°C. After equilibrium was reached, 1.6 moles of H₂O2 remained. What is Ke for the reaction?arrow_forwardAt 2000 °C the equilibrium constant for the reaction 2NO(g) = N2(g) + O2(g) is Kc = 2.4 x 10³. Part A If the initial concentration of NO is 0.175 M, what is the equilibrium concentration of NO? Express your answer to two significant figures and include the appropriate units. -4.8.10² Submit Part B X Incorrect; Try Again; 4 attempts remaining Value Submit If the initial concentration of NO is 0.175 M, what is the equilibrium concentration of N₂? Express your answer to two significant figures and include the appropriate units. Part C 0 UA M Previous Answers Request Answer Submit Value ΠΑ Units Request Answer If the initial concentration of NO is 0.175 M, what is the equilibrium concentration of O2? Express your answer to two significant figures and include the appropriate units. www ? Units Request Answer ? **** ?arrow_forwardThe Keq for the equilibrium below is 7.52 × 10-2 at 480.0 °C. 2Cl2 (g) + 2H2O (g) 4HCl (g) + O2 (g)What is the value of Keq at this temperature for the following reaction?2HCl (g) + O2 (g) Cl2 (g) + H2O (g) A) 13.3B) 3.65C) -0.0376D) 5.66 × 10-3E) 0.274arrow_forward
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