For the equilibrium reaction N2(g) + 3H2(g) 2NH3(g) DH = -92 kJ,Describe how the equilibrium concentration of N2(g) will beaffected by:(i.e. increase/decrease/no change)>>decreasing the volume:removing H₂adding Ni as a catalyst:decreasing the pressureDOraising the temperature:decreasing the volume:removing H₂adding Ni as a catalyst:((decreasing the pressureraising the temperature:reducing the [NH3]1. Increase2. Decrease3. No Change1. Increase2. Decrease3. No Change

Answered: Image /qna-images/answer/a89aff38-5695-4d15-b1f2-9921bcd8cc6b.jpg

For the equilibrium reaction N2(g) + 3H2(g) « 2NH3(g) DH = -92 kJ, Describe how the equilibrium concentration of N₂(g) will be affected by: (i.e. increase/decrease/no change) **** > > decreasing the volume: removing H₂ adding Ni as a catalyst: decreasing the pressure raising the temperature: decreasing the volume: removing H₂ adding Ni as a catalyst: decreasing the pressure raising the temperature: reducing the [NH3] 1. Increase 2. Decrease 3. No Change 1. Increase 2. Decrease 3. No Change

For the equilibrium reaction N2(g) + 3H2(g) « 2NH3(g) DH = -92 kJ, Describe how the equilibrium concentration of N₂(g) will be affected by: (i.e. increase/decrease/no change) **** > > decreasing the volume: removing H₂ adding Ni as a catalyst: decreasing the pressure raising the temperature: decreasing the volume: removing H₂ adding Ni as a catalyst: decreasing the pressure raising the temperature: reducing the [NH3] 1. Increase 2. Decrease 3. No Change 1. Increase 2. Decrease 3. No Change

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 89AP

See similar textbooks

Similar questions

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.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
Methanol can be synthesized by means of the equilibriumreaction CO(g)+2H2(g)CH3OH(g) for which the equilibrium constant at 225°C is 6.08103. Assume that the ratio of the pressures of CO(g) and H2(g) is 1:2. What values should they have if the partial pressureof methanol is to be 0.500 atm?
12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial concentrations are [O3]=1.0106M,[NO]=1.0105M,[NO2]=2.5104M, and [O2]=8.2103M , is the system at equilibrium? If not, in which direction does the reaction proceed? (b) If the temperature is increased, as on a very warm day, will the concentrations of the products increase or decrease? (HINT: You may have to calculate the enthalpy change for the reaction to find out if it is exothermic or endothermic.)
Consider the system A(g)+2B(g)+C(g)2D(g)at 25C. At zero time, only A, B, and C are present. The reaction reaches equilibrium 10 min after the reaction is initiated. Partial pressures of A, B, and D are written as PA, PB, and PD. Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required). (a) PD at 11 min PD at 12 min. (b) PA at 5 min PA at 7 min. (c) K for the forward reaction K for the reverse reaction. (d) At equilibrium, K Q. (e) After the system is at equilibrium, more of gas B is added. After the system returns to equilibrium, K before the addition of B K after the addition of B. (f) The same reaction is initiated, this time with a catalyst K for the system without a catalyst the system with a catalyst. (g) K for the formation of one mole of D K for the formation of two moles of D. (h) The temperature of the system is increased to 35C. PB at equilibrium at 25C PB at equilibrium at 35C. (i) Ten more grams of C are added to the system. PB before the addition of C PB after the addition of C.
The following data are for the system A(g)2B(g) (a) How long does it take the system to reach equilibrium? (b) How does the rate of the forward reaction compare with the rate of the reverse reaction after 30 s? After 90 s?
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.
5.2. What is the difference between a static equilibrium and a dynamic equilibrium? Give examples difference from the examples in the text. What is similar for the two types of equilibria?
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?