Concept explainers
Urea (H2NCONH2) is used extensively as a nitrogen source in fertilizers. It is produced commercially from the reaction of ammonia and carbon dioxide:
Ammonia gas at 223°C and 90. atm flows into a reactor at a rate of 500. L/min. Carbon dioxide at 223°C and 45 atm flows into the reactor at a rate of 600. L/min. What mass of urea is produced per minute by this reaction assuming 100% yield?
Trending nowThis is a popular solution!
Chapter 5 Solutions
Chemistry
- 97 Homes in rural areas where natural gas service is not available often rely on propane to fuel kitchen ranges. The propane is stored as a liquid, and the gas to be burned is produced as the liquid evaporates. Suppose an architect has hired you to consult on the choice of a propane tank for such a new home. The propane gas consumed in 1.0 hour by a typical range burner at high power would occupy roughly 165 L at 25°C and 1.0 atm, and the range chosen by the client will have six burners. If the tank under consideration holds 500.0 gallons of liquid propane, what is the minimum number of hours it would take for the range to consume an entire tankful of propane? The density of liquid propane is 0.5077 kg/L.arrow_forwardA cylinder of compressed gas is labeled Composition (mole %): 4.5% H2S, 3.0% CO2, balance N2. The pressure gauge attached to the cylinder reads 46 atm. Calculate the partial pressure of each gas, in atmospheres, in the cylinder.arrow_forwardA homeowner uses 4.00 × 103 m3 of natural gas in a year to heat a home. Assume that natural gas is all methane, CH4, and that methane is a perfect gas for the conditions of this problem, which are 1.00 atm and 20 °C. What is the mass of gas used?arrow_forward
- References Use the References to access important values if needed for this question. Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCI(aq) ZnCl2(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 754 mm Hg. If the wet H2 gas formed occupies a volume of 6.46 L, the number of moles of Zn reacted was mol. The vapor pressure of water is 23.8 mm Hg at 25 °C. Submit Answerarrow_forwardMost of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas wells. In the first step of this synthesis, called the Claus process, hydrogen sulfide gas is reacted with dioxygen gas to produce gaseous sulfur dioxide and water. Suppose a chemical engineer studying a new catalyst for the Claus reaction finds that 592. liters per second of dioxygen are consumed when the reaction is run at 195. °℃ and the dioxygen is supplied at 0.48 atm. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.arrow_forward[References) Use the References to access important values if needed for this question. Sodium metal reacts with water to produce hydrogen gas according to the following equation: 2Na(s) + 2H,0(1)2N2OH(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 755 mm Hg. If the wet H2 gas formed occupies a volume of 5.20 L, the number of moles of Na reacted was mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.arrow_forward
- In order to produce solid iron, it first must bc processed from its orc, Fe2O1, in a blast furnace. During operation, CO gas (flue gas) is introduced into the furnace at 1650 °C and a pressure of 250 kPa. In this process flue gas reduces iron to its elemental form in the following reaction: 41. Fe;O30) COg Fe+ COz At one point in this process 256.0 L of CO was used to reduce iron ore. Assuming a complete reaction, how many grams of solid iron can be produced. Balanced chemical equation: Mass of Fe (in grams)arrow_forwardSome commercial drain cleaners use a mixture of sodium hydroxide and aluminum powder. When the solid mixture is poured into the drain and dissolves, a reaction ensues that produces hydrogen gas: 2NAOH(aq) + 2Al(s) + 6H20() - 2NAAI(OH)4(aq) + 3H2(g) Determine the pressure (in kPa) of hydrogen gas produced when 39.82 g of aluminum reacts with excess sodium hydroxide and water if the temperature is 38.17 C and the volume is 7.22 L. Provide your answer with TWO decimals.arrow_forwardConsider the following situation: You have a 50 L tank of compressed air at 15 atm and 100 ºC. You then pass the compressed air through a "titanium getter" which contains fragments of hot titanium metal. The purpose of the "getter" is to remove oxygen gas from the sample as Ti reacts with oxygen to form solid TiO2 (known as titania). Once the purified air is passed through the getter is it cooled back down to 100 ºC and fills another 50 L storage tank. If air typically contains about 20% oxygen, what could the pressure in the storage tank be? Question 2 options: A) 12 atm B) 15 atm C) 18 atm D) 24 atmarrow_forward
- Urea (H2NCONH2) is used extensively as a nitrogen source in fertilizers. Itis produced commercially from the reaction of ammonia and carbon dioxide: Ammonia gas at 223°C and 90. atm flows into a reactor at a rate of 500. L/min. Carbon dioxide at 223°C and 45 atm flows into the reactor at a rate of 600. L/min. What mass of urea is produced per minute by this reaction assuming 100% yield?arrow_forwardReferences Use the References to access important values if needed for this question. Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2Al(s) + 2NAOH(aq)+ 6H2O(1)–→2NAAI(OH)4(aq) + 3H2(g) The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 757 mm Hg. If the wet H2 gas formed occupies a volume of 9.31 L, the number of grams of H, formed is g. The vapor pressure of water is 17.5 mm Hg at 20 °C. Submit Answerarrow_forwardNitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. A.) Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin ( C3H5(NO3)3 ) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. B.) Suppose 79.0L of carbon dioxide gas are produced by this reaction, at a temperature of −8.0°C and pressure of exactly 1 atm . Calculate the mass of nitroglycerin that must have reacted in grams. Round your answer to 3 significant digitsarrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning