O KINETICS AND EQUILIBRIUM Solving problems that mix equilibrium ideas with gas laws DEN Sulfuric acid is essential to dozens of important industries from steelmaking to plastics and pharmaceuticals. More sulfuric acid is made than any other industrial 11 kg per year chemical, and world production exceeds 2.0 x 10 The first step in the synthesis of sulfuric acid is usually burning solid sulfur to make sulfur dioxide gas. Suppose an engineer studying this reaction introduces 1.0 kg of solid sulfur and 10.0 atm of oxygen gas at 700. °C into an evacuated 65.0 L tank. The engineer believes p 0.14 for the reaction at this temperature. Calculate the mass of solid sulfur she expects to be consumed when the reaction reaches equilibrium. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken in her belief about the value of K and the consumption of sulfur you calculate may not be what she actually observes. kg ? Explanation Check X

O KINETICS AND EQUILIBRIUM Solving problems that mix equilibrium ideas with gas laws DEN Sulfuric acid is essential to dozens of important industries from steelmaking to plastics and pharmaceuticals. More sulfuric acid is made than any other industrial 11 kg per year chemical, and world production exceeds 2.0 x 10 The first step in the synthesis of sulfuric acid is usually burning solid sulfur to make sulfur dioxide gas. Suppose an engineer studying this reaction introduces 1.0 kg of solid sulfur and 10.0 atm of oxygen gas at 700. °C into an evacuated 65.0 L tank. The engineer believes p 0.14 for the reaction at this temperature. Calculate the mass of solid sulfur she expects to be consumed when the reaction reaches equilibrium. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken in her belief about the value of K and the consumption of sulfur you calculate may not be what she actually observes. kg ? Explanation Check X

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter5: Gases

Section: Chapter Questions

Problem 5.105PAE: 105 The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so...

See similar textbooks

Similar questions

94 Mining engineers often have to deal with gases when planning for the excavation of coal. Some of these gases, including methane, can be captured and used as fuel to support the mining operation. For a particular mine, 2.4 g of CH4 is present for every 100.0 g of coal that is extracted. If 45.6% of the methane can be captured and the daily production of the mine is 580 metric tons of coal, how many moles of methane could be obtained per day?
Methanol (CH3OH) can be produced by the following reaction: CO(g)+2H2(g)CH3OH(g) Hydrogen at STP flows into a reactor at a rate of 16.0 L/min. Carbon monoxide at STP flows into the reactor at a rate of 25.0 L/min. If 5.30 g methanol is produced per minute, what is the percent yield of the reaction?
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.
When two cotton plugs. one moistened with ammonia and the other with hydrochloric acid, are simultaneously inserted into opposite ends of a glass tube that is 87.0 cm long, a white 1111g of NH4Cl forms where gaseous NH3 and gaseous HC1 first come into contact. NH3(g)+HCl(g)NH4Cl(s) At approximately what distance from the ammonia moistened plug does this occur? (Hint: Calculate the rates of diffusion for both NH3 and HCI, and find out how much faster NH3 diffuses than HCI.)
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.