O Using the equilibrium shown below, fill in the table showing which way each stress would shift things to re-establish equilibrium and the effect on the value of Kc each stress will have. Assume that only the stress that is being applied is happening to the system at equilibrium and nothing else changes (e.g. the volume of the container remains constant unless you are told otherwise). AH = -60 kJ 2CHCI3(g) +Cl2(g) = 2CC14(1) + H2(g) Change in the value of Кс Direction of shift to re- Stress establish equilibrium Add Cl2e) Add CCl40) Remove CHCI3(g) Cool System Add a catalyst Reduce volume Add Heg)

O Using the equilibrium shown below, fill in the table showing which way each stress would shift things to re-establish equilibrium and the effect on the value of Kc each stress will have. Assume that only the stress that is being applied is happening to the system at equilibrium and nothing else changes (e.g. the volume of the container remains constant unless you are told otherwise). AH = -60 kJ 2CHCI3(g) +Cl2(g) = 2CC14(1) + H2(g) Change in the value of Кс Direction of shift to re- Stress establish equilibrium Add Cl2e) Add CCl40) Remove CHCI3(g) Cool System Add a catalyst Reduce volume Add Heg)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.83PAE

See similar textbooks

Similar questions

What would be the equilibrium temperature if you drop 5.0 g of brass (Cp = 0.38 J/g-oC, initially at 68oC) and 3.5 g of aluminum (Cp = 0.9 J/g-oC, initially at 83oC) into 105 g of water (Cp = 4.184 J/g-oC,initially at 23oC)?
The following system is at equilibrium in a closed vessel: 2 NH3(g) + 3 I2(g) ⇆ N2(g) + 6 HI(g) Various stresses are applied to the system as illustrated in the chart. Drag the appropriate label from the list below that indicates how the system responds to each stress. Each label can be used more than once.
Are the chlorine atoms in equivalent environments in each of the compounds [Co(NH3)4Cl2] and [Co(NH3)3Cl3]?
9O2 + 2P3 yields 6PO3 What would the pressure be if there are 2.75 moles of each gas in a 2.31 L container at 451 C at equilibrium and then 2.5 moles of gaseous PO3 were added to the container? Assume temperature and volume are constant What would the new pressure inside container be?
3.What would be the equilibrium temperature if you drop 5.0 g of brass (Cp = 0.38 J/g-oC, initially at 68oC) and 3.5 g of aluminum (Cp = 0.9 J/g-oC, initially at 83oC) into 105 g of water (Cp = 4.184 J/g-oC, initially at 23oC)?
Exactly 1.0 mol N2O4 is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N2O4(g) 2NO2(g). If at equilibrium the N2O4 is 28.0% dissociated, what is the value of the equilibrium constant, Kc, for the reaction under these conditions? (need to show your calculation.)
Nitrogen dioxide reacts to form dinitrogen tetroxide as follows: 2 NO2 (g) ⇌ N2O4 (g) At 327 °C, Kp = 2.89. If one starts with 10.0 atm NO2 (g), what is the equilibrium pressure (in atm) of NO2 (g)?
#343434. Exactly 3.5 moles of N2O4 are placed in an empty 2.0-L container and allowed to reach equilibrium described in the equation: N2O4(g) ⇌ 2NO2(g), at 0.58 equilibrium constant, 25% of the N2O4 will be dissociated. True False
What would be the equilibrium temperature if you drop 5.0 g of brass (Cp= 0.38 J/g-°C, initially at 68°C) and 3.5 g of aluminum (Cp = 0.9 J/g-°Cinitially at 83°C) into 105 g of water (Cp = 4.184 J/g-°C,initially at 23°C)?
a )Write out the expression for the Keq for the following reaction and determine the Keq value using the given equilibrium data. 2NH3 (g) + 185 kJ ----> N2(g) + 3H2(g) [N2]eq= 2.0 mol/L [H2]eq= 3.0 mol/L [NH3]eq = 5.0 mol/L b) For the reaction in part A) determine the way the reaction will shift with the following stresses (R = shift right, L = shift left, N = NO shift) I) Adding N2(g). _____________________________ II) Increasing the temperature. _____________________________ III) Decreasing the volume of the container. _____________________________ IV) Adding a catalyst. _____________________________ V) Removing H2(g). _____________________________
Given the Equation: 2C(g) + 2D(g) = 3E(g) + F(g) + heat ,Predict the direction of the shift in equilibrium, Removal of compound Ea. FORWARDb. BACKWARDc. NO CHANGEGiven the Equation: 2C(g) + 2D(g) = 3E(g) + F(g) + heat ,Predict the direction of the shift in equilibrium, Increase in pressurea. farwardb. backwardc. no change Given the Equation: 2C(g) + 2D(g) = 3E(g) + F(g) + heat ,Predict the direction of the shift in equilibrium, Increase in temperaturea. forwardb. backwardc. no change
Expain the dynamic equilibrium.