Homework 4Question 9 of 30 (1 point) | Question Attempt: 1 of 3✓ 2✓ 3✓ 4✓ 56✓ 7✓ 8= 91011Given this reaction at 25 °C.PCl5(g) = PC13(g) + Cl₂ (g)CompoundCl₂ (g)PCl₂ (g)PC15 (g)Initial Partial Pressure(atm)0.3060.2340.00330Use the table of initial partial pressure to find:Note: Reference the Thermodynamic properties of pure substances and Fundamental constants tables for additional information.Part 1 of 2Round your answer to 1 significant digit.Кр=21.7பx10Part 2 of 2☑Round your answer to 3 significant digits.CheckAG = -7.628kJmol☐ x10☐Save For LaterSubr

Given: T=25°CP,atmPCl5(g)0.00330⇌PCl3(g)0.234+Cl2(g)0.306Step 1: Write the equilibrium…

Answered: Homework 4 Question 9 of 30 (1 point) |…

Living by Chemistry

2nd Edition

ISBN:9781464142314

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Publisher:Angelica M. Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

Section: Chapter Questions

Problem 13STP

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A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.
Consider the formation of HI(g) from H2(g) and I2(g). H2(g)+I2(g)2HI(g) For this reaction, K at 333C is 98, while K at 527C is 62.5. Find S for I2(g) at 527C.
Data in the table were collected at 540 K for the following reaction: CO(g) + NO2(g) CO2(g) + NO(g) Using the data in the table: (a) Determine the reaction order with respect to each reactant. (b) Derive the rate equation. (c) Calculate the rate constant, giving the correct units for k.
Sodium sulfate 10-hydrate, Na2SO410H2O, dehydrates according to the equation Na2SO410H2O(s)Na2SO4(s)+10H2O(g)KP=4.081025 at 25 C What is the pressure of water vapor at equilibrium with a mixture of Na2SO410H2O and NaSO4?
The equilibrium constant K for the reaction 2CI(g)CI2(g) was measured as a function of temperature (Kelvin). A graph of In (K) versus 1/T for this reaction gives a straight line with a slope of 1.352 104 K and a y-intercept of 14.5 1. Determine the values of H and S for this reaction. See Exercise 79.
5.22. True or false: If for a gas-phase reaction, then all equilibrium partial pressures of reactants and products must equal . Explain your choice.
For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273 K. If one starts with 0.3 atm of CO2 and 12.0 g of C at 1273 K, will the equilibrium mixture contain (a) mostly CO2? (b) mostly CO? (c) roughly equal amounts of CO2 and CO? (d) only C?
Predict the temperature at which the reaction in Exercise 17.67 comes to equilibrium. Consider the equation G = H TS. At some value of T, G equals zero and the reaction is at equilibrium. Set G = 0, substitute for H and S (assuming that they do not vary much with temperature) and solve for T. CH3CHO(l)+52O2(g)2CO2(g)+2H2O(l)
Consider the following reaction at some temperature: H2O(g)+CO(g)H2(g)+CO2(g)K=2.0 Some molecules of H2O and CO are placed in a 1.0-L container as shown below. When equilibrium is reached, bow many molecules of H2O, CO, H2, and CO2 are present? Do this problem by trial and error-that is, if two molecules of CO react, is this equilibrium; if three molecules of CO react, is this equilibrium; and so on.
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
Consider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial pressure of CO2 at room temperature?
For the decomposition of Ag2O: 2Ag2O(s)4Ag(s)+O2(g)(a) Obtain an expression for G as a function of temperature. Prepare a table of G values at 100 K intervals between 100 K and 500 K. b) Calculate the temperature at which G =0.

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