11.17 Ammonia can react with oxygen to produce nitric oxide and water:
If the rate at which ammonia is consumed in a laboratory experiment is 4.23 ×10-4 mol L_1s_l, at what rate is oxygen consumed? At what rate is NO produced? At what rate is water vapor produced?
Trending nowThis is a popular solution!
Chapter 11 Solutions
Chemistry for Engineering Students
- Silicon forms a series of compounds analogous to the al-kanes and having the general formula SinH2n+2. The first of these compounds is silane, SiH4, which is used in the electronics industry to produce thin ultrapure silicon films. SiH4(g) is somewhat difficult to work with because it is py-ropboric at room temperature—meaning that it bursts into flame spontaneously when exposed to air. (a) Write an equation for the combustion of SiH4(g). (The reaction is analogous to hydrocarbon combustion, and SiO2 is a solid under standard conditions. Assume the water produced will be a gas.) (b) Use the data from Appendix E to calculate ? for this reaction. (c) Calculate G and show that the reaction is spontaneous at 25°C. (d) Compare G for this reaction to the combustion of methane. (See the previous problem.) Are the reactions in these two exercises enthalpy or entropy driven? Explain.arrow_forwardAmoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small animals, the pharmacist or veterinarian must suspend it in water, so that it can be administered orally with a medicine dropper. The label says to dispose of unused suspension after 14 days. It also points out that refrigeration is required. In the context of this chapter, what is implied in the latter two statements?arrow_forward7. Sulfuryl chloride, SO2Cl2, is a highly reactive gaseous compound. When heated, it decomposes as follows: SO2Cl2 (g) ⇌ SO2 (g) + Cl2 (g). This decomposition is endothermic. A sample of 3.509 grams of SO2Cl2 is placed in an evacuated 1.00-L bulb and the temperature is raised to 375 K. a. What would be the pressure (in atm) in the bulb if no dissociation of the SO2Cl2(g) occurred? b. When the system has come to equilibrium at 375 K, the total pressure in the bulb is found to be 1.43 atm. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium. c. Give the expression for the equilibrium constant (either Kp or KC) for the decomposition of SO2Cl2(g) at 375 K. Calculate the value of the equilibrium constant you have selected. d. If the temperature were raised to 500 K, what effect would this have on the equilibrium constant? Explain in 1-2 sentences.arrow_forward
- Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 309. liters per second of dioxygen are consumed when the reaction is run at 217.°C and 0.70atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.arrow_forward1) Sulfuryl chloride, SO2Cl2, is a highly reactive gaseous compound. When heated, it decomposes as follows: SO2Cl2(g) ® SO2(g) + Cl2(g). This decomposition is endothermic. A sample of 3.509 grams of SO2Cl2 is placed in an evacuated 1.00 liter bulb and the temperature is raised to 375K. (a) What would be the pressure in atmospheres in the bulb if no dissociation of the SO2Cl2(g) occurred? (b) When the system has come to equilibrium at 375K, the total pressure in the bulb is found to be 1.43 atmospheres. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium at 375K. Note: Please answer both A and Barrow_forward1) Sulfuryl chloride, SO2Cl2, is a highly reactive gaseous compound. When heated, it decomposes as follows: SO2Cl2(g) ® SO2(g) + Cl2(g). This decomposition is endothermic. A sample of 3.509 grams of SO2Cl2 is placed in an evacuated 1.00 liter bulb and the temperature is raised to 375K. (a) What would be the pressure in atmospheres in the bulb if no dissociation of the SO2Cl2(g) occurred? (b) When the system has come to equilibrium at 375K, the total pressure in the bulb is found to be 1.43 atmospheres. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium at 375K. (c) Give the expression for the equilibrium constant (either Kp or Kc) for the decomposition of SO2Cl2(g) at 375K. Calculate the value of the equilibrium constant you have given, and specify its units. (d) If the temperature were raised to 500K, what effect would this have on the equilibrium constant? Explain briefly. Note: Please answer just C and D. Thank you.arrow_forward
- In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas to produce gaseous ammonia. This reaction is now the first step taken to make most of the world's fertilizer. Suppose a chemical engineer studying a new catalyst for the Haber reaction finds that 960. liters per second of dinitrogen are consumed when the reaction is run at 189. °C and the dinitrogen is supplied at 0.74 atm. Calculate the rate at which ammonia is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.arrow_forwardConsider the reaction: NO2(g) + CO(g) -->NO(g) + CO2(g). Could you follow the progress of this reaction by monitoring the pressure of the gas in the container in which it was occurring?arrow_forwardA bimolecular chemical reaction is one in which two chemicals react to form another substance. Suppose that one molecule of each of the two chemicals reacts to form two molecules of a new substance. If x represents the number of molecules of the new substance at time t, then the rate of change of x is proportional to the square of the numbers of molecules of the original chemicals available to be converted. That is, if each of the chemicals initially contained A molecules, then dx dt = k(A − x)2 where k is a constant. If 40% of the initial amount A is converted after 1 hour, how long will it be before 50% is converted? (Give an exact answer. Do not round.)arrow_forward
- I was told to repost this question, because I got the explanations for a-c. I just need d explained. 7. Sulfuryl chloride, SO2Cl2, is a highly reactive gaseous compound. When heated, it decomposes as follows: SO2Cl2 (g) ⇌ SO2 (g) + Cl2 (g). This decomposition is endothermic. A sample of 3.509 grams of SO2Cl2 is placed in an evacuated 1.00-L bulb and the temperature is raised to 375 K. a. What would be the pressure (in atm) in the bulb if no dissociation of the SO2Cl2(g) occurred? b. When the system has come to equilibrium at 375 K, the total pressure in the bulb is found to be 1.43 atm. Calculate the partial pressures of SO2, Cl2, and SO2Cl2 at equilibrium. c. Give the expression for the equilibrium constant (either Kp or KC) for the decomposition of SO2Cl2(g) at 375 K. Calculate the value of the equilibrium constant you have selected. d. If the temperature were raised to 500 K, what effect would this have on the equilibrium constant? Explain in 1-2 sentences.arrow_forwardOne reaction that occures in an automobile catalytic converter is the conversion of nitrogen monoxide to nitrogen and oxygen. 2NO(g) --> N2(g) + O2(g) A) write the relative rates of consumption and formation using the balanced equation. B) If the rate is 0.250 M/s over the first 5.50 s, how much NO(g) will be consumed?arrow_forwardOne reaction that occurs in an automobile catalytic converter is the conversion of nitrogen monoxide to nitrogen and oxygen. 2NO(g) ---> N2(g) + O2(g) A) write the relative rates of consumption and formation using the balanced equation. B) If the rate is 0.25 M/s over the first 5.50 s, how much NO(g) will be consumed?arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning