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: Orise ☐ O 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 Ono ☐ atm

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: Orise ☐ O 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 Ono ☐ atm

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...

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Use thermochemical data given in the table to decide whether the equilibrium constant for each of the following reactions will increase or decrease with temperature. Substance AH; (kJ/mol) CO(g) CO₂ (g) CS₂(g) CH₁ (9) H₂(g) H₂S(g) H₂O(g) N₂ (9) NH3 (9) O₂(g) -111 -394 117 -74.9 0 -20.5 -242 0 -45.9 0 a. CO₂(g) + H₂(g) → CO(g) + H₂O(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase. b. 2CO2 (g) 2CO(g) + O2(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase.
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 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: 2NO, (g) – N,04(g) AG = - 5.4 kJ Now suppose a reaction vessel is filled with 7.26 atm of dinitrogen tetroxide (N,O) at 95. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N,O, tend to rise or fall? 4 fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,0, will tend to rise, can that yes be changed to a tendency to fall by adding N0,? Similarly, if you said the no pressure of N,0, will tend to fall, can that be changed to a tendency to rise by adding NO,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO, needed to reverse it. atm Round your answer to 2 significant digits. O O
For the following reaction, AH = 2816 kJ. 6 CO₂(g) + 6 H₂O(I) ⇒ C6H12O6(s) + 6 O₂(g) Select ONE combination of strategies that when applied to this system at equilibrium will result in an increase in the amount of C6H₁2O6 as equilibrium is re-established? a. Increasing Po₂ by adding more O2; increasing the temperature; decreasing the volume; or removing CO₂ b. Increasing Po₂ by adding more O₂ and decreasing the volume C. Decreasing the volume d. Increasing Po₂ by adding more O₂ e. Increasing the temperature
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.
At -8.64 °C the concentration equilibrium constant K = 7.7 for a certain reaction. Here are some facts about the reaction: -1 • The initial rate of the reaction is 5.3 mol·L¯¹·s¯¹. . If the reaction is run at constant pressure, 132. kJ/mol of heat are absorbed. • The constant pressure molar heat capacity C = 2.97 J'mol K¹. Yes. Using these facts, can you calculate K at 16. °C? x10 O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat 16. °C will be bigger or smaller than K at -8.64 °C? C Yes, and K will be bigger. Yes, and K will be smaller. No.
17. The thermochemical equation for the reaction of F2 and water is as follows. AH = -270 kJ F2(g) + 2 H2O (liq)=HF (aq) + O2 (g) Given a system that is initially at equilibrium, which of the following actions cause the reaction to proceed to the right? a) adding O2(g) b) decreasing the temperature c) adding a catalyst d) decreasing the volume of the reaction chamber e) none of the above
Use the tabulated information to calculate the equilibrium constant (K) for for the following reaction, at 25°C. R= 8.314 J/mol.K 2HNO3(aq) + NO (g) → ) 3NO,(g) +H,O(l) NO (g) NO₂ (g) H₂O (1) AG() 87.6 51.3 -237.1 O 5.11 z 10-4 O 1.15 x 10-9 O 1.02 O 8.71 x 108 O 9.80 HNO3(aq) -110.9
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
Consider the system N2(g) + 3 Cl2(g) 2 NCI3(g) AH = +232 kJ Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by each of the following. decreasing the temperature removing nitrogen trichloride gas 1. forward reaction compressing the system at constant temperature 2. reverse reaction adding chlorine gas