At - 19.4 °C the pressure equilibrium constant K = 6.3 x 10' for a certain reaction.Here are some facts about the reaction:• The net change in moles of gases is -1.If the reaction is run at constant pressure, the volume increases by 12.%.If the reaction is run at constant pressure, 138. kJ/mol of heat are released.○ Yes.Using these facts, can you calculate K, at -26. °C?○ No.If you said yes, then enter your answer at right. Round it to2 significant digits.atIf you said no, can you at least decide whether K-26. °C will be bigger or smaller than K,, at -19.4 °C?0Yes, and K,, will bebigger.Yes, and K, will besmaller.○ No.X

The objective is to calculate the equilibrium constant pressure.Given:Pressure equilibrium constant…

At - 19.4 °C the pressure equilibrium constant Kp = 6.3 × 10° for a certain reaction. Here are some facts about the reaction: The net change in moles of gases is -1. If the reaction is run at constant pressure, the volume increases by 12.%. • If the reaction is run at constant pressure, 138. kJ/mol of heat are released. Using these facts, can you calculate K, at -26. °C? O Yes. ○ No. If you said yes, then enter your answer at right. Round it to 2 significant digits. at If you said no, can you at least decide whether K -26. °C will be bigger or smaller than K at - 19.4 °C? | Yes, and Kp bigger. will be Yes, and K, will be No. smaller.

At - 19.4 °C the pressure equilibrium constant Kp = 6.3 × 10° for a certain reaction. Here are some facts about the reaction: The net change in moles of gases is -1. If the reaction is run at constant pressure, the volume increases by 12.%. • If the reaction is run at constant pressure, 138. kJ/mol of heat are released. Using these facts, can you calculate K, at -26. °C? O Yes. ○ No. If you said yes, then enter your answer at right. Round it to 2 significant digits. at If you said no, can you at least decide whether K -26. °C will be bigger or smaller than K at - 19.4 °C? | Yes, and Kp bigger. will be Yes, and K, will be No. smaller.

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

A reaction is studied at various temperatures, and a graph of ln K ( equilibrium constants on y axis) versus 1/T (Temperature on x axis) is prepared in Excel. The equation of the line is found to be y = - 9500 x + 21.5. What is the ΔSfor this reaction in J/mol/K? (assume R=8.314Jmol⋅K)
Using any data you can find in the ALEKS Data resource, calculate the quilibrium constant K at 25.0°C for the following reaction. Fe2O3(s)+ 3H2(g)→ 2Fe(s)+ 3H2O(l) Round your answer to 2 significant digits. delta G of Fe2O3=-742.2 kj/mol h2=0 Fe=0 H20=-237.1kj/mol
Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free energy of formation values can be found in this table. 3 NO₂(g) + H₂O(1) – 2 HNO3 (1)+NO(g) -52.83 kJ/mol AGTxn Incorrect
Consider the following equilibrium: N2 (g)+3H2(g)2NH3 (g) AG = -34. kJ Now suppose a reaction vessel is filled with 2.15 atm of nitrogen (N2) and 2.19 atm of ammonia (NH3) at 236. °C. Answer the following questions about this system: OO rise ☐ x10 fall OO Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H2? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm S
Consider the following equilibrium: N2O4(g) 2NO2 (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 2.78 atm of dinitrogen tetroxide (N204) at 710. °C. Answer the following questions about this system: rise x10 fall Under these conditions, will the pressure of N2O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm X S
At -5.92 °C the pressure equilibrium constant K = 5.9 for a certain reaction. P Here are some facts about the reaction: • If the reaction is run at constant pressure, 127. kJ/mol of heat are released. • The constant pressure molar heat capacity C • The net change in moles of gases is -1. = 2.41 J mol -1. K¹. -1 р Yes. ☐ x10 Using these facts, can you calculate K at -27. °C? ○ No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Р If you said no, can you at least decide whether K at -27. °C will be bigger or smaller than K, at −5.92 °C? П Yes, and K, will be р bigger. Yes, and K smaller. will be No. ☑
Consider the reaction: PbCl2(s) → Pb2*(aq) + 2 Cl (aq) AH° = 23.30 kJ/mol and AS° = -12.5 J/K-mol a) When solid PbCl2 is dissolved in water at 25°C, what are the concentrations of Pb2* and Cl at equilibrium? (Hint: Do your ICE chart and Law of Mass Action.) Concentration of Pb2+: mol/L and Concentration of Cl = mol/L (Do not use superscripts, subscripts, or carets. Write 1.2 x 10-3 as 1.2x10-3 or 1.2e-3.) b) At 25°C, This reaction is (reactant or product) favored. Justify your answer with the appropriate calculation on the separate sheet of paper. c) The Gibbs free energy at 25°C, when both the concentrations of the lead ion and chloride ion are 1.2 x 10-³M is kJ/mol. Show your calculations on the separate sheet of paper.
Consider the following equilibrium: 2NH3(g) = N₂ (g) + 3H₂(g) 2 AG = 34. kJ Now suppose a reaction vessel is filled with 7.87 atm of ammonia (NH3) and 1.17 atm of hydrogen (H₂) at 448. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise 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. Round your answer to 2 significant digits. rise fall yes no atm x10 X 5
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
We start with a sample of pure A(g). The following equilibrium is established 2 A(g) <---> B(g) + C(g) The total pressure is 8.33 atm and the temperature is 25.0oC. The partial pressure of A(g) is 5.26 atm. Calculate the value of the standard free enthalpy change (in kJ) of this reaction at 25.0oC.
Consider the reaction in the Haber process 3H2 (g) + N2 (g) → 2NH3 (g)where delta H° = -91.8 kJ/mol and delta S° = -197 J/(mol*K). What is the value of the equilibrium constant (K) at a temperature of 125°C?
Consider the following equilibrium: 2NO₂(g) → N₂O4 (g) AG = -5.4 kJ Now suppose a reaction vessel is filled with 0.202 atm of nitrogen dioxide (NO₂) at 504. °C. A Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O4? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O4? Similarly, if you said the pressure of NO₂ will tend to fall, can that be changed to a tendency to rise by adding N₂O4? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O needed to reverse it. V Round your answer to 2 significant digits. Orise fall O yes no atm 0