Ch.10 - Gases: Their Properties & Behavior
Chapter 10, Problem 77
Assume that you have 1.00 g of nitroglycerin in a 500.0-mL steel container at 20.0 °C and 1.00 atm pressure. An explosion occurs, raising the temperature of the container and its contents to 425 °C. The balanced equation is 4 C3H5N3O91l2¡ 12 CO21g2 + 10 H2O1g2 + 6 N21g2 + O21g2 (c) What is the pressure in atmospheres inside the container after the explosion according to the ideal gas law?
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Textbook Question
Titanium(III) chloride, a substance used in catalysts for preparing polyethylene, is made by high-temperature reaction of TiCl4 vapor with H2: 2 TiCl4(g) + H2(g) → 2 TiCl3(s) + 2 HCl(g) (a) How many grams of TiCl4 are needed for complete reaction with 155 L of H2 at 435 °C and 795 mm Hg pressure?
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Textbook Question
Titanium(III) chloride, a substance used in catalysts for preparing polyethylene, is made by high-temperature reaction of TiCl4 vapor with H2: 2 TiCl4(g) + H2(g) → 2 TiCl3(s) + 2 HCl(g) (b) How many liters of HCl gas at STP will result from the reaction described in part (a)?
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Textbook Question
A typical high-pressure tire on a bicycle might have a volume of 365 mL and a pressure of 7.80 atm at 25 °C. Suppose the rider filled the tire with helium to minimize weight. What is the mass of the helium in the tire?
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Textbook Question
Natural gas is a mixture of many substances, primarily CH4, C2H6, C3Hg, and C4H10. Assuming that the total pressure of the gases is 1.48 atm and that their mole ratio is 94:4.0:1.5:0.50, calculate the partial pressure in atmospheres of each gas.
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Textbook Question
A special gas mixture used in bacterial growth chambers contains 1.00% by weight CO2 and 99.0% O2. What is the partial pressure in atmospheres of each gas at a total pressure of 0.977 atm?
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Textbook Question
What is the mole fraction of each gas in the mixture described
in Problem 10.83?
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