For the gas-phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25 °C, it is found that the partial pressure of C is 0.210 atm. What is AGO for this reaction? (R = 8.314 J/mol·K).

For the gas-phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25 °C, it is found that the partial pressure of C is 0.210 atm. What is AGO for this reaction? (R = 8.314 J/mol·K).

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

N2(g) + 3H2 (g) = 2NH3 (g) AH°pn =-92 kJ Which of the following changes would cause the value of K for this reaction to increase? You can choose any combination of answers. Decreasing the volume of the reaction container. Heating the reaction container Cooling the reaction container Adding Helg) to the reaction container removing NH3(g) from reaction container.
At -7.73 °C the pressure equilibrium constant K, =6.8 × 10° for a certain reaction. Here are some facts about the reaction: • The constant pressure molar heat capacity C, 1.76 J·mol -1. K¯!. • If the reaction is run at constant pressure, the volume increases by 14.%. The initial rate of the reaction is 11. mol·L - 1 -1 •S O Yes. Using these facts, can you calculate K, at 15. °C? O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K, will be bigger. If you said no, can you at least decide whether K at Yes, and K, will be 15. °C will be bigger or smaller than K, at -7.73 °C? smaller.
The following reaction takes place into a constant-volume flask at 427°C: CCL(g) = C(s) +2 C2(g) AH=132 kJ At 427°C, the equilibrium constant for the reaction given above is K. = 1.3×10-2. A flask is filled with 2.00 atm of CCl4 at 427°C. (a) What is the value of K for this reaction? (R=0.082 L.atm/mol.K) (b) What are the partial pressures of CClL, Ch and the total pressure at equilibrium? (c) How will the equilibrium pressure of CCl(g) change if the temperature is increased? (d) How will the equilibrium system respond if the volume of the flask is reduced?
Determine the final temperature of a reaction that was initially 25 C, given that its equilibrium constant tripled and the reaction’s enthalpy of formation is 60.15 kJ/mol.
Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into 5.00 L flask. The flask is found to contain 8.62 g of CO, 2.60 g of H2, 43.0 g of CH4, and 48.4 g of H:O at 320.0 °C. What are the values of Kc and Kp for this reaction? CH:(g) + H2O(g) = CO(g) + 3 H2(g) 1 2 NEXT > Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms.
Nitric oxide reacts with chlorine to form NOCI. 2NO(g) + Cl2g) → 2NOCI(g) The equilibrium constant K at 298K is x 107. (R = 8.314 J/K • mol) Substance: NO(g) Cl2g) NOCIG) AH°F (k]/mol) at 298 K 90.29 51.71 S°U/K• mol) at 298 K 210.65 223.0 261.60
For the reaction below, what is the effect of raising the temperature? 4A(g) + B(g) 3C(g) AH = - 405 kJ Equilibrium shifts to the right; the reaction makes more products. O The reaction makes more of both products and reactants, so equilibrium is unaffected O Equilibrium re-establishes Equilibrium shifts to the left; the reaction makes more reactants.
Heating HI(g) at 425 °C causes some of this compound to decompose, forming H2 (g) and I2 (g). Eventually, the amounts of the three species do not change further, the system has reached equilibrium. (At this point, approximately 22% of the HI has decomposed.) What is happening in this system at the molecular level? O H2(g) reacts with I2 (g) to produce HI(g) at the same rate as it decomposes. H2 (g) and I2 (g) molecules collide with HI(g) making the reaction stop. Only part of the HI(g) molecules has enough energy to decompose at this temperature. 5:55 PM FLV 2/22/2020 Type here to search hp ins prt sc delete home f12 f8 f9 f10 f5 f6 f7 14 10 num & backspace lock 23 8. 3 %24
Consider the following equilibrium: N,0, (g) = 2NO, (3) AG' = 5.4 kJ Now suppose a reaction vessel is filled with 0.496 atm of nitrogen dioxide (NO,) at 137. °C. Answer the following questions about this system: O rise Under these conditions, will the pressure of NO, tend to rise or fall? O fall Is it possible to reverse this tendency by adding N,O,? In other words, if you said the pressure of NO, will tend to rise, can that O yes be changed to a tendency to fall by adding N,04? Similarly, if you said O no the pressure of NO, will tend to fall, can that be changed to a tendency to rise by adding N,0,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N,0, needed to reverse it. O atm Round your answer to 2 significant digits.
Consider the following equilibrium: N₂ (g) + 3H₂(g)2NH₂ (g) AG = -34. KJ 2 Now suppose a reaction vessel is filled with 3.70 atm of hydrogen (H₂) and 8.46 atm of ammonia (NH3) at 1099. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of H ₂ tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding N₂? x Ś ? In other words, if you said the pressure of H₂ will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the yes no pressure of H₂ will tend to fall, can that be changed to a tendency to rise 2 by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. atm Round your answer to 2 significant digits. ● O
8. Consider the equilibrium reaction: N2(g) + O2(g) = 2 NO(g) Kp 4.10 x 10³ at 2000°C a) If 1.00 atm of nitrogen gas and 1.00 atm of oxygen gas is mixed with 0.10 atm of nitrogen monoxide in a 500.0 mL container at 2000°C, in which direction will the reaction proceed to reach equilibrium? Show all work to justify your answer. b) What is the concentration of each gas when equilibrium is reached at 2000°C? Show all your work. Equilibrium Partial Pressures: PN₂ = Po₂ = 1.02 atm and PNO = 0.07 atm Use PV = nRT Answer: Equilibrium Concentrations: [N₂] = [0₂] = 5.47 x 10-3 mol/L and [NO] = 4 x 10+ M
For the gas-phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25°C, it is found that the partial pressure of C is 0.270 atm. What is AG° for this reaction? (R = 8.314 J/mol · K). kJ/mol 1 3 4 C 7 8 9 +/- x 100 + 2.