To calculate the quantity of argon present in 1 L of air and to calculate the volume of air required to isolate 1 mol of argon at 1 atm pressure and 25 ∘ C . Concept introduction: The pressure exerted by an individual gas in a mixture is known as its partial pressure. Dalton’s law of partial pressure states that the total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases; P Total = P 1 + P 2 + P 3 + ... Dalton’s law can also be expressed using the mole fraction of gases, x ; P 1 = x ( P Total ) (1) The Ideal gas equation is written as, PV = n RT (2) Here, The pressure of the gas is P The volume of the gas is V The gas constant is R The total number of moles is n The temperature of the system is T
To calculate the quantity of argon present in 1 L of air and to calculate the volume of air required to isolate 1 mol of argon at 1 atm pressure and 25 ∘ C . Concept introduction: The pressure exerted by an individual gas in a mixture is known as its partial pressure. Dalton’s law of partial pressure states that the total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases; P Total = P 1 + P 2 + P 3 + ... Dalton’s law can also be expressed using the mole fraction of gases, x ; P 1 = x ( P Total ) (1) The Ideal gas equation is written as, PV = n RT (2) Here, The pressure of the gas is P The volume of the gas is V The gas constant is R The total number of moles is n The temperature of the system is T
Solution Summary: The author explains Dalton's law of partial pressure, which states that the total pressure of a mixture of gases is equal to the sum of the partial
To calculate the quantity of argon present in 1L of air and to calculate the volume of air required to isolate 1mol of argon at 1atm pressure and 25∘C.
Concept introduction:
The pressure exerted by an individual gas in a mixture is known as its partial pressure.
Dalton’s law of partial pressure states that the total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases;
PTotal=P1+P2+P3+...
Dalton’s law can also be expressed using the mole fraction of gases, x;
A mixture of xenon and fluorine was heated. A sample of the white solid that formed reacted with hydrogen to yield 81 mL of xenon (at STP) and hydrogen fluoride, which was collected in water, giving a solution of hydrofluoric acid. The hydrofluoric acid solution was titrated, and 68.43 mL of 0.3172 M sodium hydroxide was required to reach the equivalence point. Determine the empirical formula for the white solid and write balanced chemical equations for the reactions involving xenon.
The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium azide, which produces large volumes
of nitrogen gas.
1. Write a balanced chemical equation, including physical state symbols, for the
decomposition of solid sodium azide (NaN) into solid sodium and gaseous dinitrogen.
dlo
2. Suppose 12.0 L of dinitrogen gas are produced by this reaction, at a temperature of
13.0 °C and pressure of exactly 1 atm. Calculate the mass of sodium azide that must
have reacted. Round your answer to 3 significant digits.
Explanation
Check
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Solid molybdenum(VI) oxide reacts with gaseous xenon difluoride to form liquid molybdenum(VI) fluoride, xenon gas, and oxygen gas. Write the Qc for this reaction.
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