The production capacity for acrylonitrile (C3H3N) in the United States is over 2 billion pounds per year. Acrylonitrile, the building block for polyacrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen 2C3H6(g) + 2NH3(g) + 302(g) → 2C3H3N(g) + 6H₂O(g) Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: Mass 4.74x10² g propylene 5.00 x 102 g ammonia 1.00 x 103 g oxygen Reactant What mass of water is formed from your mixture? mass of water formed = g Calculate the mass (in grams) of each reactant after the reaction is complete: oxygen g= mass of acrylonitrile produced Reactant Mass remaining propylene ammonia Submit Show Hints g 9 9 Previous Next

The production capacity for acrylonitrile (C3H3N) in the United States is over 2 billion pounds per year. Acrylonitrile, the building block for polyacrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen 2C3H6(g) + 2NH3(g) + 302(g) → 2C3H3N(g) + 6H₂O(g) Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: Mass 4.74x10² g propylene 5.00 x 102 g ammonia 1.00 x 103 g oxygen Reactant What mass of water is formed from your mixture? mass of water formed = g Calculate the mass (in grams) of each reactant after the reaction is complete: oxygen g= mass of acrylonitrile produced Reactant Mass remaining propylene ammonia Submit Show Hints g 9 9 Previous Next

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3 and water: 2Al(OH)3(s) + Al2O3(s) -> 3H2O(g) In the second step, alumina Al2O3 and carbon react to form aluminum and carbon dioxide: 2Al2O3(s) + 3C(s) + 4Al(s) -> 3CO2(g) Suppose the yield of the first step is 74.% and the yield of the second step is 76.% . Calculate the mass of aluminum hydroxide required to make 4.0kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
Silicon nitride (Si3N4) is a desirable ceramic material that withstands hightemperatures. Si3N4 can be produced by reacting silicon tetrachloride (SiCl4) withammonia (NH3). In addition to Si3N4, hydrogen chloride (HCl) is produced in thisreaction. There are no other reactants or products.(Molecular masses: Si3N4 = 140.31 g/mol, SiCl4 = 169.7 g/mol, NH3 = 17.03 g/mol)a. Please write a balanced equation for this reaction.______________________________________________b. If 128.0 g of SiCl4 is reacted with 10.2 g of NH3, which of these twocompounds is the limiting reactant for the production of Si3N4?_______________c. How much excess reagent (in grams) is left? ______________
10 Ethylene (CH,CH,) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 10º kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH,CH,) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 60.0 L reaction tank with 22.0 atm of ethane gas and raises the temperature to 500. °C. She believes K =0.050 at this temperature. Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken about the correct value of K , and the mass percent of ethylene you calculate may not be what she actually observes. %
One method used in the production of H2 gas is to put the coal into an incomplete combustion reaction with air and water vapor in the combustion chamber (water gas production). A simplified reaction can be written as:2C + 1 H2O + a (O2+3.76N2) = 1C0 + 1CO2 + 1H2 + 3.76·a·N2 Here, 02+3.76N2 represents the amount of air and is multiplied by the coefficient "a".a) The value of the coefficient "a" for this reaction b) The amount of air to be used for 1 kg of pure carbon (C) (total amount of 02 and N2) (kg-air/kg-carbon) Hint: Consider how many kilograms 1 kmol "C" weighs.
A materials scientist has created an alloy containing aluminum, copper, and zinc, and wants to determine the percent composition of the alloy. The scientist takes a 12.849 g sample of the alloy and reacts it with concentrated HCl. The reaction converts all of the aluminum and zinc in the alloy to aluminum chloride and zinc chloride in addition to producing hydrogen gas. The copper does not react with the HCl. Upon completion of the reaction, a total of 10.4 L of hydrogen gas was collected at a pressure of 724 torr and a temperature of 27.0 °C. Additionally, 2.836 g of unreacted copper is recovered. Calculate the mass of hydrogen gas formed from the reaction. mass: ----- g Calculate the mass of aluminum in the alloy sample. mass: ---- g What is the mass percent composition of the alloy? Cu: -----% Zn: ----% Al: -----%
Consider the following reactions:CoO (s) + CO (g) D CO2 (g) + Co (s) Kc(1) = 490.2 CoO (s) + 2 H2 (g) D 2 Co (s) + 2 H2O (g) Kc(2) = 4.5 x 103a. Write the overall equation for the reaction of hydrogen gas and carbon dioxide gas to produce carbon monoxide gas and steam.
In one sentence explain what's wrong with this equation, and rewrite it so that the coefficients are correct. C3H6(g)+4.5 O2(g)->3CO2(g)+3H2O(g)
Automakers are always investigating alternative reactions for the generation of gas to inflate air bags, in part because the sodium produced in the decomposition of NaN3 presents safety concerns. One system that has been considered is the oxidation of graphite by strontium nitrate, Sr(NO3)2, as shown in the equation below. 5 C(s) + 2 Sr(NO3)2 (8)→ 2 SrO(s) + 2 N₂(g) + 5 CO₂(g) Suppose that a system is being designed using this reaction, and the goal is to generate enough gas to inflate a bag to 63 L and 1.4 atm at 23°C. What is the minimum mass of graphite that should be used in the design of this system? g C(s)
Ammonia (NH3) is an important compountd is used in large amounts for the manufacture of nitrogenous fertilizers, nylon and many other important compounds. It is manufactured by the catalytic reaction between nitrogen between nitrogen and hydrogen, according to the following equation; N2(g) +H2(g) = NH;(g) When 1.20 mol nitrogen and 1.20 mol hydrogen are mixed together in a closed vessel, 30% of the nitrogen is converted into ammonia. a. Calculate the moles of nitrogen gas that will be present in the vessel? (only 3 decimal places) mol b. Calculate the moles of hydrogen gas that will be present in the vessel? (only 3 decimal places) mol c. Calculate the moles of ammonia gas that will be present in the vessel? (only 3 decimal places) Activate W mol d. What is the number of moles of nitrogen gas that has reacted? (only 3 decimal places) 10:09 Links 18°C 1O 23-Nov-21
Mercury is an environmental pollutant because it can be converted by certain bacteria into the very poisonous substance dimethyl mercury, (CH3)2Hg. This compound ends up in the food chain and accumulates in the tissues of aquatic organisms, particularly fish, which renders them unsafe to eat. It is estimated that in the United States, 241 tons of mercury are released into the atmosphere each year. If only 1.9 percent of this mercury is eventually changed to (CH3)2Hg, how many pounds of this compound are formed annually?
10 Ethylene (CH,CH,) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 10° kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH,CH,) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 25.0 L reaction tank with 20.0 atm of ethane gas and raises the temperature to 650. °C. He believes =0.040 at this temperature. K,= Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken about the correct value of K, and the mass percent of ethylene you calculate may not be what he `p' actually observes.
4. A common experiment at Science Fairs is the demonstration of a volcano using a mixture of baking soda, NaHCO3(s), and vinegar, CH₂COOH(aq), with the reaction: NaHCO3(s) + CH3COOH(aq)- CO2(g) + H₂O(l) + Nat(aq) + CH3COO(aq) where the heavier CO2 gas displaces the liquid mixture to the top of the container to simulate lava overflowing. If the volume of the reaction vessel is 0.500 L and the pressure is 0.997 atm and 298 K. given 50.5 ml of 0.351 M CH3COOH() in water, what mass of NaHCO3(s) is required to fill the bottle with CO2 gas?