3. For the following reaction, write how the each of the changes will affect the indicated quantity, assuming a container of fixed size. Write "increase", "decrease", or "no change". (Or use an "up" arrow to indicate "increase", and a "down" arrow to indicate "decrease".) (For a chemical added, write how it would respond AFTER the addition.) H2(g) + Br2(g) 2HBI(g) AH° = -103.7kJ %3D [HBr] K value Change Some H, added [H] [Br3] 1. 2. Some HBr added 3. Some H removed 4. Some HBrremoved S The temperature is increased 6. The temperature is decreased 7. Pressure is increased and the container volume decreased

3. For the following reaction, write how the each of the changes will affect the indicated quantity, assuming a container of fixed size. Write "increase", "decrease", or "no change". (Or use an "up" arrow to indicate "increase", and a "down" arrow to indicate "decrease".) (For a chemical added, write how it would respond AFTER the addition.) H2(g) + Br2(g) 2HBI(g) AH° = -103.7kJ %3D [HBr] K value Change Some H, added [H] [Br3] 1. 2. Some HBr added 3. Some H removed 4. Some HBrremoved S The temperature is increased 6. The temperature is decreased 7. Pressure is increased and the container volume decreased

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

Initially 10.0 mol of ammonia gas is injected into a 4.0 L container. At equilibrium 1.2 mol of nitrogen gas is found in the container. The number of moles of ammonia gas at equilibrium would be? 2NH3(g) + 94 kJ <=====> N2(g) + 3H2(g)
For the reaction 2 NO2 (g) <-=> N2O4 (g) , Kp =_____ Kc(RT) Kc/RT (RT)/Kc Kc
What may happen to the reaction rate when you add catalyst on it? Choose from the choices below: It increased It decreased, then increased It decreased It did not change
Volume of HCI (mL) Volume of NaOH (mL) Temperature of HCI (°C) Temperature of mixture after reaction (°C) Temperature difference (°C) Number of joules evolved (J) (enter a positive value) Moles of H* that were neutralized (mol) Joules evolved per mole of H* (J/mol) Trial 1 50.0 50.0 27.4 31.8 4.4 X Ⓒ x Trial 2 50.0 50.0 27.4 31.8 4.4
Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10-4 M. N2(g) + 3H2(g) = 2NH3(g) Ton: N. x10-2 ent (O Pncca waythe chemical system would 5 the vara BI U = E T O Word(s) ------ T T; O Word(s) 5. If the concentration of the product NH3 was increased from 1.0x 10-4 M to 5.6 x 10-3 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. B I U E T O Word(s)
Can you show me how to answer this type of question I found on a online practice organic chemistry review.
Please answer ALL parts of the question and show your work. Consider this reaction: 2H2S(g) + 3O2(g) <-----> 2H2O(g) + 2SO2(g) H= -1036 kJ Predict whether the forward or reverse reaction will reestablish equilibrium is disturbed by (a) expanding the container (b) removing SO2 (c) rasing the temperature (d) water vapor is added
Given the UNBALANCED equilibrium equation: A (g) + B2 (g) AB ( g) Which is the correct equilibrium expression? [A]²[B]! Keg = %3D [AB]? [AB]? Keq = [A]² [B]? (AB]? Keq %3D [A]? [B]! [A]*[B]? [AB]? Keq = %3D [AB]! Keq = [A] [B]?
Use the following PE diagram to answer the following questio PE (kJ) 100 80 60 40 20 A + B C + D Progress of the reaction Is the reaction exothermic or endothermic? Exothermic Endothermic You need more information.
3- Negative enthalpy means Oa- The reaction absorbs heat. b- The reaction doesn't absorb or evolve heat. d- The reaction depend on concentrations. the reaction evolve heat
For the reaction: N2(g) + 3H2(g) 2NH3(g) + heat If the reaction were allowed to reach equilibrium and you were to add heat, what would happen? [Check all that are correct.] Equilibrium would shift to the right. Equilibrium would shift to the left. The amount of N2 would increase. The amount of H2 would increase. O The amount of NH3 would increase.
Consider the following reaction for this question Cl₂, H₂O