Part ACarbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reactionIf only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium?Express your answer with the appropriate units.▸ View Available Hint(s)for Part A for Part A do for Part redo for Part A resel for Part A keyboard shortcuts for Part A help for Part A[COF2] = 0.32Submit Previous AnswersPart BX Incorrect; Try Again; 5 attempts remainingMConsider the reaction, which takes place at a certain elevated temperaturefor Part B for Part B do for Part redo for Part B res@for Part B keyboard shortcuts for Part B help for Part B|HCONH2] = |0.501If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will the concentration of HCONH2 be at equilibrium?Express your answer with the appropriate units.► View Available Hint(s)Submit Previous AnswersM2COF2 (g) = CO2 (g) + CF4(g), Kc = 8.00X Incorrect; Try Again; 5 attempts remainingCO(g) + NH3(g) =HCONH₂(g), K = 0.840 Part BThe following reaction was carried out in a 2.00 L reaction vessel at 1100 K:If during the course of the reaction, the vessel is found to contain 6.75 mol of C, 12.6 mol of H₂O, 3.40 mol of CO, and 6.30 mol of H₂, what is the reaction quotient Qc?Enter the reaction quotient numerically.► View Available Hint(s)Qc =for Part B for Part do for Part redo for Part B resetor Part B keyboard shortcuts for Part B help for Part BSubmitC(s) + H₂O(g) = CO(g) + H₂(g)

concentration of COF2 concentration of HCONH2 Qc

▾ Part A Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction If only COF₂ is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium? Express your answer with the appropriate units. ▸ View Available Hint(s) [COF2] 0.32 for Part A for Party do for Part redo for Part A reor Part A keyboard shortcuts for Part A help for Part A M Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining Part B Consider the reaction, which takes place at a certain elevated temperature Submit If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will the concentration of HCONH₂ be at equilibrium? Express your answer with the appropriate units. ▸ View Available Hint(s) for Rprt B for Part.do for Part redo foart B resor Part B keyboard shortcuts for Part B help for Part B M [HCONHz)= |0.501 2COF2 (g) CO2(g) + CF4(g), Ke= 8.00 Previous Answers CO(g) + NH3(g) = HCONH₂(g), K = 0.840

▾ Part A Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction If only COF₂ is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium? Express your answer with the appropriate units. ▸ View Available Hint(s) [COF2] 0.32 for Part A for Party do for Part redo for Part A reor Part A keyboard shortcuts for Part A help for Part A M Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining Part B Consider the reaction, which takes place at a certain elevated temperature Submit If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will the concentration of HCONH₂ be at equilibrium? Express your answer with the appropriate units. ▸ View Available Hint(s) for Rprt B for Part.do for Part redo foart B resor Part B keyboard shortcuts for Part B help for Part B M [HCONHz)= |0.501 2COF2 (g) CO2(g) + CF4(g), Ke= 8.00 Previous Answers CO(g) + NH3(g) = HCONH₂(g), K = 0.840

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 105CWP: In a given experiment, 5.2 moles of pure NOCl was placed in an otherwise empty 2.0-L container....

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1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L"' ofO2, what were the equilibrium concentrations of all species?
Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was injected into a 5.0-L container at 2500 K, at which the equilibrium constant is 3.6 X 10-?. What was the composition of the reaction mixture at equilibrium? l'he following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
Write the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)
A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.
In a given experiment, 5.2 moles of pure NOCl was placed in an otherwise empty 2.0-L container. Equilibrium was established by the following reaction: 2NOCl(g)2NO(g)+Cl2(g)K=1.6105 a. Using numerical values for the concentrations in the Initial row and expressions containing the variable x in both the Change and Equilibrium rows, complete the following table summarizing what happens as this reaction reaches equilibrium. Let x = the concentration of Cl2 that is present at equilibrium. b. Calculate the equilibrium concentrations for all species.
Hydrogen, bromine, and HBr in the gas phase are in equilibrium in a container of fixed volume. H2(g) + Br2(g) 2 HBr(g) rH = 103.7 kJ/mol How will each of these changes affect the indicated quantities? Write increase, decrease, or no change.
Mustard 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?
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer
For a typical equilibrium problem, the value of K and the initial reaction conditions are given for a specific reaction, and you are asked to calculate the equilibrium concentrations. Many of these calculations involve solving a quadratic or cubic equation. What can you do to avoid solving a quadratic or cubic equation and still come up with reasonable equilibrium concentrations?
The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N2 and O2 being injected into a 1.0-L container at 2500 K. The equilibrium constant at 2500 K is 3.6 X 10“’. What was the composition of the reaction mixture after equilibrium was attained? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?