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Exam 5: Gases

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Question 41

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Define Charles's Law

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The volume of a fixed amount o...

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Question 42

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Phosgene, a chemical warfare agent used in World War I, consists of 12.41% C, 16.17% O, and 71.69% Cl.1.00 L of this gas at STP has a mass of 4.42 g.What is the molecular formula of phosgene?

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Baking powder is made up of sodium hydrogen carbonate and calcium hydrogen phosphate.When baking powder is wet, these components react to produce carbon dioxide.The equation for this reaction is given below. NaHCO₃(aq)+ CaHPO₄(aq) $\rarr$ NaCaPO₄(aq)+ CO₂(g)+ H₂O(l) Assuming all of the carbon dioxide was released as a gas, how many liters of CO₂(g)would be formed at room temperature from 4.00 g of NaHCO₃ and excess CaHPO₄?

A 0.271 g sample of an unknown vapor occupies 294 mL at 140.°C and 847 mmHg.The empirical formula of the compound is CH₂.What is the molecular formula of the compound?

At constant temperature, the volume of the container that a sample of nitrogen gas is in is doubled.As a result the pressure of the nitrogen gas is halved.The amount of nitrogen gas is unchanged in this process.This is an example of:

Calculate the volume of H₂(g) at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride.

A 1.17 g sample of an alkane hydrocarbon gas occupies a volume of 674 mL at 28°C and 741 mmHg.Alkanes are known to have the general formula CnH2n+2.What is the molecular formula of the gas in this sample? (R = 0.08206 L.atm/K.mol)

A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21°C is allowed to rise to the stratosphere where the temperature is -5°C and the pressure is 1.0 millibar.What is the final volume of the balloon in Liters? 1.000 atm = 1.013 bar.

A 45 mL sample of nitrogen gas is cooled from 135ºC to 15°C in a container that can contract or expand at constant pressure, what is the new volume of the nitrogen gas?

A 707 mg sample of a gas containing only carbon and oxygen occupies a volume of 452 mL at 63 °C and 745 mmHg.Identify the gas in the sample.(R = 0.08206 L.atm/K.mol)

An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm.If the can contains 1.0 g CO₂ and is heated to 400°C, will it burst?

The molecules of different samples of an ideal gas have the same average kinetic energies, at the same

A sample of hydrogen gas was collected over water at 21°C and 685 mmHg.The volume of the container was 7.80 L.Calculate the mass of H₂(g) collected.(Vapor pressure of water = 18.6 mmHg at 21°C.)

Calculate the volume occupied by 25.2 g of CO₂ at 0.84 atm and 25°C.R = 0.08206 L.atm/K.mol.

Which of these gases will have the greatest density at the same specified temperature and pressure?

Determine the pressure of the gas trapped in the apparatus shown below when the atmospheric pressure is 695 mmHg.

A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm³; the density of water is 1.00 g/cm³.

A particular coal sample contains 2.32% S.When the coal is burned, the sulfur is converted to sulfur dioxide gas.What volume (L)of SO₂(g), measured at 25°C and 749 mmHg, is produced by burning 2.0 × 10⁶ lb of this coal? (1 lb = 454 g)

At constant temperature and volume, a sample of oxygen gas is added to a sample of nitrogen gas.The pressure of the mixture is found by adding the pressures of the two individual gases.This is an example of:

What is the pressure (mmHg)of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 742 mmHg and h = 16.7 cm?