Practice ProblemATTEMPT
Write the reaction quotient for each of the following reactions:
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Chemistry
Additional Science Textbook Solutions
Chemistry: Atoms First
Living By Chemistry: First Edition Textbook
Introductory Chemistry (6th Edition)
General, Organic, & Biological Chemistry
Organic Chemistry
Chemistry: The Central Science (14th Edition)
- 5. Dinitrogen pentoxide is added to an evacuated rigid container at 25°C. Given that the initial pressure is 1.00 atm and at equi- librium the pressure is 0.500 atm, determine the final pressure in the reaction vessel at equilibrium. 2N2O5(g) = 4NO2(g) + O2(8) (A) 0.750 atm (B) 1.00 atm (C) 1.25 atm (D) 1.75 atmarrow_forward1.1 1 (a) N₂(g) = + 180 kJ mol-¹ + O₂(g) (b) Increasing the pressure From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (c) Increasing the temperature (d) Increasing the concentration of N₂ (e) Adding a catalyst 2NO (g) ΔΗ, 298arrow_forwardThe reaction N2O4(g) =* 2NO2(g) has a K, = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N2O4 was 0.279 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO2= i atm (b) What was the total pressure of the mixture of gases? total pressure = i atmarrow_forward
- Calculate AGO for each of the following reactions from the equilibrium constant at the temperature given. (a) N2(g) + O2(g) (b) H2(g) + I2(g) 2NO(g) 2HI(g) (c) CO2(g) + H2(g) → CO(g) + H2O(g) (d) CaCO3(s) →CaO(s) + CO2 (g) T = 2000 °C K₁ = 4.1 × 10-4 T = 400 °C Кр = $50.0 T = 980 °C T = 900 °C Кр Кр = 1.67 = 1.04 K₁ = 7.2 × 10-4 (e) HF(aq) + H2O(l) → H3O+ (aq) + F¯(aq) T = 25 °C (f) AgBr(s) → Ag+ (aq) + Br(aq) T = 25 °C Kp = 3.3 × 10-13arrow_forwardThe reaction N₂O4(g) 2NO₂(g) has a Kp = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N₂O4 was 0.344 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO₂ = atm (b) What was the total pressure of the mixture of gases? total pressure = atmarrow_forwardA flask is charged with 1.720 atm of N₂O4(g) and 0.88 atm NO₂(g) at 25°C. The equilibrium reaction is given in the equation below. N₂04(9) 2NO₂(g) After equilibrium is reached, the partial pressure of NO₂ is 0.512 atm. (a) What is the equilibrium partial pressure of N₂O4? 1.904 atm (b) Calculate the value of K, for the reaction. 0.137 (c) Is there sufficient information to calculate K for the reaction? O Yes, because the partial pressures of all the reactants and products are specified. Ⓒ Yes, because the temperature is specified. O No, because the value of K. can be determined experimentally only. If K can be calculated, find the value of K. Otherwise, enter 0. 2.30e-4 Xarrow_forward
- What is the correct value of the equilibrium constant Kc for the reaction: 2 NH3(g) N₂(g) + 3 H₂(g) Given that is Kc = 10 at T = 740 K for: N₂(g) + 3 H₂(g) (A) more information needed (B) 0.01 (C) 100 (D) 0.1 (E) 10 = = 2 NH3(g)arrow_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_forwardWhat effect does an increase in pressure have on each of the following systems at equilibrium? The temperature is kept constant and, in each case, the reactants are in a cylinder fitted with a movable piston. (a) A(s) 2B(s) (b) 2A(1) B(1) (c) A(s) B(g) (d) A(g) = B(g) (e) A(g) 2B(g)arrow_forward
- Consider the following equilibrium for which H = 180.74: N2(g) + O2(g) 2 NO(g) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction?(a) NO(g) is added to the system. (b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%. (d) A catalyst is added to the reaction mixture. (e) The total pressure of the system is increased by adding a noble gas. (f) O2(g) is removed from the system.arrow_forward(b) At 100° C, the Keq for the Haber process is 4,51 X 10-5: N₂ + 3 H₂ 2 NH3 Consider the following reaction conditions and determine if the system is at equilibrium. If not, indicate the direction in which the reaction must proceed to establish equilibrium (i) PNH3 105 atm, PN2 = 35 atm and PH2 = 495 atm (ii) PNH3 35 atm, PN2 = 0 atm and PH2 = 595 atm (iii) PNH3 = 26 atm, PN2 = 202 atm and PH2 = 42 atm (iv) PNH3 105 atm, PN2 = 5 atm and PH2 = 55 atmarrow_forwardA(s) + B(g) ⇋2 C (g) For each of the statements below, identify whether it is true or false and explain why. (a)All else equal, increasing the total pressure will favor the forward reaction. (b)All else equal, adding excess A to the reaction will favor the forward reaction. (c)All else equal, adding excess B to the reaction will favor the forward reaction. (d)If higher temperature leads to a decrease in total pressure, the forward reaction must be exothermic. (e)If higher temperature leads to an increase in total pressure, the forward reaction must be endothermic.arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY