Indicate how each of the following will affect the equilibrium concentration of
a. adding more
b. increasing the temperature
c. increasing the volume of the container
d. adding more
e. removing some
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Basic Chemistry
- At 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_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_forwardWhich change causes the equilibrium to shift to the product side? 2 CO) + O2(2) 2 CO2(2) AH= - (3)0) 283.3kJ (3)2) (3)2) ORemoving oxygen O Increasing the temperature O Adding carbon dioxide Removing carbon monoxide Decreasing the volumearrow_forward
- The enthalpy change in the reaction: N2O (g) + NO2 (g) ⇄3 NO (g)is +115.7 kJ / mol. Will the direction of the equilibrium shift LEFT, RIGHT, or STAY THE SAME when the following stresses are applied to the system?(12a): Removing nitrogen dioxide gas(12b): Adding dinitrogen monoxide gas(12c): Adding nitrogen monoxide gas(12d): Decreasing the volume of the system(12e): Increasing the temperaturearrow_forwardLe Chatelier’s principle states that “If you stress a system at equilibrium, the system will react to relieve the stress and return to equilibrium”. The following equation represents a chemical reaction at equilibrium: 2A (g) + 3B (g) <===> 2C (g) + 4D (g) ∆H = -378 kcal/mol (g) means gas In each case below, explain how the system reacts (forward direction, reverse direction or no change): The concentration of A is increased Heat is added to the system B is removed from the reaction Pressure is added The concentration of C is increasedarrow_forward4:15 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_forward
- 10. 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_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_forward4 (a) Calculate the value of Kc for the reaction: PCI5 (g) PC13 (g) Cl2 (g) AH = Positive Given that when 8.4 mol of PCI5 (g) is mixed with 1.8 mol of PCI3 (g) and allowed to come to equilibrium in a 10 dm³ container the amount of PCI5 (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: (i) Increasing temperature (ii) Lowering the concentration of chlorine (Cl2) (iii) Addition of a catalystarrow_forward
- 4. When nitrogen gas and chlorine gas react to form nitrogen trichloridge gas, an equilibrium is established in which Keq = 4.15 x 10-5 at 200°C. N₂ (g) + 3 Cl₂ (g) — 2 NCI3 (9) If 2.74 mol of nitrogen gas, N₂ (g), and 0.84 mol of chlorine gas, Cl₂ (g), are put in a 2.0 L reaction vessel, what is the equilibirum concentration of the nitrogen trichloride gas, NC13 (g) at this temperature?arrow_forwardFlag 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_forward7 4 (a) Calculate the value of Kc for the reaction: PC15 (2) PC13 (g) + Cl2 (g) AH = Positive Given that when 8.4 mol of PCls (g) is mixed with 1.8 mol of PC13 (g) and allowed to come to equilibrium in a 10 dm³ container the amount of PCls (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: (1) Increasing temperature (ii) Lowering the concentration of chlorine (Cl2) (iii) Addition of a catalystarrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning