7. Gases

Standard Temperature and Pressure

7. Gases

Standard Temperature and Pressure

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Standard Temperature and Pressure

Standard Temperature and Pressure Example 1

Standard Temperature and Pressure

Standard Temperature and Pressure Example 2

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Pressure, Volume and Temperature Relationships - Chemistry Tutorial

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Pressure, Volume and Temperature Relationships - Chemistry Tutorial

What is the standard temperature and pressure STP?

Standard Temperature and Pressure Conversions

What Are Standard Conditions?

Professor Dave Explains

STP Gas Chemistry (Standard Temperature and Pressure) Examples Practice Problems Questions Shortcut

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Multiple Choice

A sample of dichloromethane gas (CH₂Cl₂) occupies 32.6 L at 310 K and 5.30 atm. Determine its volume at STP?

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Multiple Choice

Which gas sample has the greatest volume at STP?

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Multiple Choice

Nitrogen and hydrogen combine to form ammonia via the following reaction:

1 N₂ (s) + 3 H₂ (g) → 2 NH₃ (g)

What mass of nitrogen is required to completely react with 800.0 mL H₂at STP?

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Multiple Choice

What is the pressure inside a 1.5-L container that is charged with 3.0 moles of a gas at 35.0℃?

When 1 mole of gas is placed under STP conditions, what is the volume?

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Multiple Choice

The combustion of glucose yields carbon dioxide and water according to the following reaction:

C₆H₁₂O₆ (s) + 6 O₂ (g) → 6 CO₂ (g) + 6 H₂O (l)

Calculate the mass of H₂O produced when 12.0 g of glucose is combusted in a container of oxygen with a volume of 1.3 L at a pressure of 2.2 atm and a temperature of 205℃.

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Textbook Question

Propane gas 1C3H82 is often used as fuel in rural areas. How many liters of CO2 are formed at STP by the complete combustion of the propane in a container with a volume of 15.0 L and a pressure of 4.50 atm at 25.0 °C? The equation for the combustion of propane is: C3H81g2 + 5 O21g2¡3 CO21g2 + 4 H2O1l2 (LO 10.4, 10.5) (a) 61.8 L (b) 186 L (c) 20.6 L (d) 2.21 * 103 L

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Textbook Question

At standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively. (b) On cooling to 160 K, both substances form crystalline solids. Do you expect the molar volumes to decrease or increase on cooling the gases to 160 K?

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Textbook Question

At standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively. (c) The densities of crystalline Cl2 and NH3 at 160 K are 2.02 and 0.84 g/cm3, respectively. Calculate their molar volumes.

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Textbook Question

(b) What is the molar volume of an ideal gas at STP?

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Textbook Question

Chlorine is widely used to purify municipal water supplies and to treat swimming pool waters. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 119.3 kPa and 24 °C. (b) What volume will the Cl2 occupy at STP?

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Textbook Question

Many gases are shipped in high-pressure containers. Consider a steel tank whose volume is 210.0 L that contains O2 gas at a pressure of 16,500 kPa at 23 °C. (b) What volume would the gas occupy at STP?

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Textbook Question

The surface temperature of Venus is about 1050 K, and the pressure is about 75 Earth atmospheres. Assuming that these conditions represent a Venusian 'STP,' what is the standard molar volume in liters of a gas on Venus?

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Textbook Question

Which sample contains more molecules: 1.00 L of O2 at STP, 1.00 L of air at STP, or 1.00 L of H2 at STP?

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Textbook Question

A compressed air tank carried by scuba divers has a volume of 8.0 L and a pressure of 140 atm at 20 °C. What is the volume of air in the tank in liters at STP?

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Textbook Question

Use the molar volume of a gas at STP to determine the volume (in L) occupied by 33.6 g of neon at STP.

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Textbook Question

Use the molar volume of a gas at STP to calculate the density (in g>L) of nitrogen gas at STP.

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Textbook Question

Imagine that you have two identical flasks, one containing hydrogen at STP and the other containing oxygen at STP. How can you tell which is which without opening them?

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Textbook Question

One mole of an ideal gas has a volume of 22.414 L at STP. Assuming ideal behavior, what are the densities of the following gases in g/L at STP? (a) CH4 (b) CO2 (c) O2

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Textbook Question

What are the molecular weights of the gases with the following densities: (a) 1.342 g/L at STP

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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 TiCl41g2 + H21g2¡2 TiCl31s2 + 2 HCl1g2 (b) How many liters of HCl gas at STP will result from the reaction described in part (a)?

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Textbook Question

Automobile air bags inflate following a serious impact. The impact triggers the chemical reaction: 2 NaN3(s)¡2 Na(s) + 3 N2( g) If an automobile air bag has a volume of 11.8 L, what mass of NaN3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.

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Textbook Question

Lithium reacts with nitrogen gas according to the reaction: 6 Li(s) + N2( g)¡2 Li3N(s) What mass of lithium (in g) reacts completely with 58.5 mL of N2 gas at STP?

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Textbook Question

Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation: CH4( g) + H2O( g)¡CO( g) + 3 H2( g) In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25 °C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125 °C). The reaction produces 26.2 L of hydrogen gas at STP. What is the percent yield of the reaction?

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Textbook Question

Suppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (b) density?

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Textbook Question

Suppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (a) number of molecules?

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