Chapter #16 Solutions - Physical Science with Modern Applications - Melvin Merken - 5th Edition

 

1. Discuss a method that might be used to measure the rate of a reaction. Get solution

2. Although a lump of coal burns slowly, a mine full of coal dust may explode. Explain. Get solution

3. Why do iron filings burn more rapidly in pure O2 than in air? Get solution

4. Why does a 10°C rise in temperature have a marked effect on the rate of many chemical reactions? Get solution

5. Milk quickly spoils if left at room temperature but keeps for several days in a refrigerator. Explain. Get solution

6. Why do reaction rates usually increase with increasing temperatures? Get solution

7. Discuss the collision model for chemical reactions. Get solution

8. Describe how a catalyst may accelerate a chemical reaction. Get solution

9. Biochemical reactions occur in our bodies at atmospheric pressure and at about 37°C. Explain why higher pressures and temperatures are usually required to carry out similar reactions in the laboratory. Get solution

10. Methane burns vigorously in oxygen, yet a mixture of methane and oxygen can be kept indefinitely without reacting. Explain. Get solution

11. If you wished a reaction to go faster, what might you try to accomplish this? Get solution

12. What is the role of activation energy in the rate of a reaction? Get solution

13. Equilibrium represents the balancing of opposing processes. Explain why a vapor pressure above a liquid in a closed container represents an equilibrium. Get solution

14. A chemical reaction may be reversible or irreversible. How would you classify burning a piece of paper? Get solution

15. A chemical equilibrium is indicated by writing two opposing arrows, .... Explain. Get solution

16. Explain why reactants are not converted completely to products in many chemical reactions. Get solution

17. What does it mean to say that a chemical equilibrium is a dynamic system? Get solution

18. Discuss the principle of dynamic equilibrium as it applies to the system.... Get solution

19. What does the equilibrium constant for a reaction represent? Get solution

20. What do square brackets [ ] indicate when we write an equilibrium constant? Get solution

21. If the reaction...is at equilibrium, are the concentrations of NO, O2, and NO2 necessarily equal? Get solution

22. Write expressions for tire equilibrium constants of the following reactions.(a) ...(b) ...(c) ... Get solution

23. For which of the following systems does the reaction go least to completion in the forward direction: (a) K = 10−10; (b) K = 1; (c) K = 104? Get solution

24. The rocket propellant hydrazine reacts with oxygen according to the following equation:...Write the equilibrium expression. Get solution

25. Sulfur dioxide contributes to atmospheric pollution through its oxidation to sulfur trioxide:...Determine the value of the equilibrium constant, K, for this reaction if the equilibrium concentrations of a mixture of the gases areSO2 = 4.20 × 10−7 mole/literSO3 = 0.500 mole/literO2 = 2.10 × 10−7 mole/liter Get solution

26. An equilibrium constant for a reaction is 3.20 × 107. Is the formation of products of reactants favored? Get solution

27. What does Le Châtelier’s principle tell us about maximizing the yield of a reaction? Get solution

28. What change in conditions changes the equilibrium constant K of a reaction? Get solution

29. For the equilibrium system...list four ways in which the concentration of SO3 at equilibrium could be increased. Get solution

30. For the reaction...what is the effect of (a) an addition of N2? (b) an increase in temperature? (c) an increase in pressure? Get solution

31. Will an increase in temperature cause the following equilibrium system to shift to the left, shift to the right, or have no effect?... Get solution

32. Predict the effect of (a) an increase in the concentration of one reactant; (b) an increase in pressure; (c) an increase in temperature; and (d) the introduction of a catalyst upon the following reactions at equilibrium:1. ...2. ... Get solution

33. Explain how increasing the temperature would affect the equilibrium... Get solution

34. Multiple ChoiceA. Which of the following would probably slow down the rate of a reaction?(a) increasing the temperature(b) increasing the concentration(c) using a larger beaker(d) lowering the temperatureB. The principal reason for the increase in reaction rate with temperature is(a) molecules collide more frequently.(b) the pressure increases.(c) the activation energy increases.(d) the fraction of high-energy molecules increases.C. Which of the following changes will increase the yield of products at equilibrium?(a) an increase in temperature(b) an increase in pressure(c) addition of a catalyst(d) increasing reactant concentrationsD. What is the effect of increasing the concentration of B in the reaction ...?(a) the value of K decreases(b) the value of K increases(c) the equilibrium shifts to the right(d) the equilibrium shifts to the leftE. A catalyst speeds up a reaction by(a) increasing the energy released.(b) decreasing the energy released.(c) increasing the activation energy.(d) decreasing the activation energy.F. To speed up a reaction, all of the following will work except(a) increasing the concentrations of the reactants.(b) adding a suitable catalyst.(c) lowering the temperature.(d) creating more surface area by pulverizing a solid reactant.G. Which one of the following changes has no effect on the position of equilibrium?(a) an increase in temperature(b) a decrease in temperature(c) addition of a catalyst(d) addition of a productH. When a reaction has reached equilibrium,(a) all reaction ceases.(b) the rate of the forward reaction becomes zero.(c) the concentrations of reactants and products are equal.(d) the rates of the forward and reverse reactions are equal.I. The value of K for a particular reaction changes if(a) the temperature is changed.(b) the concentration is changed.(c) a catalyst is added.(d) but K never changes.J. Chemical kinetics is the study of(a) equilibrium.(b) reaction rates.(c) catalysis.(d) solutions. Get solution


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