The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1583L of nitrogen gas and 4549 L of hydrogen gas at STP, heat the mixture to run the reaction, then separate the ammonia from the reaction mixture. What volume of reactant, measured at STP, is left over in liters? Assume the reaction goes to completion. N2 (g) + 3 H2 (g) → 2 NH3 (g)

The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1583L of nitrogen gas and 4549 L of hydrogen gas at STP, heat the mixture to run the reaction, then separate the ammonia from the reaction mixture. What volume of reactant, measured at STP, is left over in liters? Assume the reaction goes to completion. N2 (g) + 3 H2 (g) → 2 NH3 (g)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter6: The Gaseous State

Section: Chapter Questions

Problem 6.72QE: Nitrogen monoxide gas reacts with oxygen gas to produce nitrogen dioxide gas. What volume of...

See similar textbooks

Similar questions

Consider the following unbalanced chemical equation: ^Sfr) + O2(g) —? Cu2O(s) + SO2(g) What volume of oxygen gas, measured at 27.5 °C and 0.998 atm. is required to react with 25 g of copper!I) sulfide? What volume of sulfur dioxide gas is produced under the same conditions?
61 As one step in its purification, nickel metal reacts with carbon monoxide to form a compound called nickel tetracarbonyl, Ni(CO)4, which is a gas at temperature above about 316 K. A 2.000-L flask is filled with CO gas to a pressure of 748 torr at 350.0 K, and then 5.00 g of Ni is added. If the reaction describe occurs and goes to completion at constant temperature, what will the final pressure in the falsk be?
Potassium peroxide is used to absorb the CO2 produced by the people in a space vehicle. 2K2O2(s)+2CO2(g)2K2CO3(s)+O2(g)If a person at rest exhales 3.0 L of air per minute and CO2 is 3.4% (by volume) of exhaled air, how many grams of K2O2 are needed per person for a five-day trip. Assume a temperature of 250 and 728 mm Hg pressure.
57 What volume of hydrogen gas, in liters, is produced by the reaction of 3.43 g of iron metal with 40.0 mL of 2.43 M HCl? The gas is collected at 2.25 atm of pressure and 23 C. The other product is FeCl2?
Hydrogen gas is used in weather balloon because it is less expensive than Helium. Assume that 5.57 g of H2 is used to fill a weather balloon to an initial volume of 67 L at 1.04 atm. If the ballloon rises to an altitude where the pressure is 0.047 atm, what is its new volume? Assume that the temperature remains constant.
A 1.26-g sample of a gas occupies a volume of 544 mL at 27 C and 744 torr? What is the molecular formula and name of the gas if its empirical formula is C2H5.
55 Ammonia is not the only possible fertilizer. Others include urea, which can be produced by the reaction: CO2(g)+2NH3(g)CO(NH2)2(s)+H2O(g) A scientist has 75 g of dry ice to provide the carbon dioxide. If 4.50 L of ammonia at 15 C and a pressure of 1.4 atm is added, which reactant is limiting? What mass of urea will form?
54 One way to generate oxygen is to heat potassium chlorate, KClO3. (The other product is potassium chloride.) If 386 mL of oxygen at 41 C and 97.8 kPa is generated by this reaction, what is the minimum mass of KClO3used?
Nitrogen monoxide gas reacts with oxygen gas to produce nitrogen dioxide gas. What volume of nitrogen dioxide is produced from the reaction of 1 L nitrogen monoxide gas with 3 L oxygen gas? What volume, if any, of the reactants will remain after the reaction ends? Assume all volumes are measured at the same pressure and temperature.
Consider the following unbalanced chemical equation: 6H12O6(s) + O2(g) -> CO,(g) + H2O(g) What volume of oxygen gas. measured at 28 °C and 0.976 atm. is needed to react with 5.00 g of C*H|2O6? What volume of each product is produced under the same conditions?
A 0.105-g sample of a gaseous compound has a pressure of 561 mm Hg in a volume of 125 mL at 23.0 C. What is its molar mass?
An organic compound contains C, H, N, and O. Combustion of 0.1023 g of the compound in excess oxygen yielded 0.2766 g CO2 and 0.0991 g H2O. A sample of 0.4831 g of the compound was analyzed for nitrogen by the Dumas method (see Exercise 129). At STP, 27.6 mL of dry N2 was obtained. In a third experiment, the density of the compound as a gas was found to be 4.02 g/L at 127C and 256 torr. What are the empirical and molecular formulas of the compound?