Concept explainers
55 Ammonia is not the only possible fertilizer. Others include urea, which can be produced by the reaction:
A scientist has 75 g of dry ice to provide the carbon dioxide. If 4.50 L of ammonia at
Trending nowThis is a popular solution!
Chapter 5 Solutions
Chemistry for Engineering Students
- You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.arrow_forwardLiquid oxygen was first prepared by heating potassium chlorate, KClO3, in a closed vessel to obtain oxygen at high pressure. The oxygen was cooled until it liquefied. 2KClO3(s)2KCl(s)+3O2(g) If 171 g of potassium chlorate reacts in a 2.70-L vessel, which was initially evacuated, what pressure of oxygen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.arrow_forwardRaoul Pictet, the Swiss physicist who first liquefied oxygen, attempted to liquefy hydrogen. He heated potassium formate, KCHO2, with KOH in a closed 2.50-Lvessel. KCHO2(s)+KOH(s)K2CO3(s)+H2(g) If 75.0 g of potassium formate reacts in a 2.50-L vessel, which was initially evacuated, what pressure of hydrogen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.arrow_forward
- Describe what happens o the average kinetic energy of ideal gas molecules when the conditions are changed as follows: (a) The pressure of the gas is increased by reducing the volume at constant temperature. (b) The pressure of the gas is increased by increasing the temperature at constant volume. (c) The average velocity of the molecules is increased by a factor of 2.arrow_forwardYou have a 550.-mL tank of gas with a pressure of 1.56 atm at 24 C. You thought the gas was pure carbon monoxide gas, CO, but you later found it was contaminated by small quantities of gaseous CO2 and O2. Analysis shows that the tank pressure is 1.34 atm (at 24 C) if the CO2 is removed. Another experiment shows that 0.0870 g of O2 can be removed chemically. What are the masses of CO and CO2 in the tank, and what is the partial pressure of each of the three gases at 25 C?arrow_forwardAmmonia gas is synthesized by combining hydrogen and nitrogen: 3 H2(g) + N2(g) 2 NH3(g) (a) If you want to produce 562 g of NH3, what volume of H2 gas, at 56 C and 745 mm Hg, is required? (b) Nitrogen for this reaction will be obtained from air. What volume of air, measured at 29 C and 745 mm Hg pressure, will be required to provide the nitrogen needed to produce 562 g of NH3? Assume the sample of air contains 78.1 mole % N2.arrow_forward
- 52 If tetraborane, B4H10, is treated with pure oxygen, it burns to give B2O3 and H2O: 2B4H10(s)+11O2(g)4B2O3(s)+10H2O(g) If a 0.050-g sample of tetraborane burns completely in O2, what will be the pressure of the gaseous water in a 4.25-L flask at 30.0 C?arrow_forwardIf equal masses of O2 and N2 are placed in separate containers of equal volume at the same temperature, which of the following statements is true? If false, explain why it is false. (a) The pressure in the flask containing N2 is greater than that in the flask containing O2. (b) There are more molecules in the flask containing O2 than in the flask containing N2.arrow_forwardUnder which of the following sets of conditions does a real gas behave most like an ideal gas, and for which conditions is a real gas expected to deviate from ideal behavior? Explain. (a) high pressure, small volume (b) high temperature, low pressure (c) low temperature, high pressurearrow_forward
- A study of climbers who reached the summit of Mount Everest without supplemental oxygen showed that the partial pressures of O2 and CO2 in their lungs were 35 mm Mg and 7.5 mm Hg, respectively. The barometric pressure at the summit was 253 mm Hg. Assume the lung gases are saturated with moisture at a body temperature of 37 C [which means the partial pressure of water vapor in the lungs is P(H2O) = 47.1 mm Hg]. If you assume the lung gases consist of only O2, N2, CO2, and H2O, what is the partial pressure of N2?arrow_forwardA typical barometric pressure in Redding. California, is about 750 mm Hg. Calculate this pressure in atm and kPa.arrow_forwardA new boron hydride, BxHy, has been isolated. To find its molar mass, you measure the pressure of the gas in a known volume at a known temperature. The following experimental data are collected: Mass of gas = 12.5 mg Pressure of gas = 24.8 mm Hg Temperature = 25 C Volume of flask = 125 mL Which formula corresponds to the calculated molar mass? (a) B2H6 (b) B4H10 (c) B5H9 (d) B6H10 (e) Bl0H14arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning