pogonofor9z
2022-01-06
Answered

A gas mixture contains $75.2\mathrm{\%}$ nitrogen and $24.8\mathrm{\%}$ krypton by mass. What is the partial pressure of krypton in the mixture if the total pressure is 745 mm Hg?

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hysgubwyri3

Answered 2022-01-07
Author has **43** answers

Use the mole fraction equation to determine the partial pressure of krypton

Jeremy Merritt

Answered 2022-01-08
Author has **31** answers

Step 1

Given data

A gas mixture contains -

Nitrogen

krypton

total pressure is 745 mmHg.

Step 2

Solution-

calculate the mole fraction of the component-

Mole fraction of tha erypton —

partial pressure of the crypton:

total pressure x mole fraction of the crypton

karton

Answered 2022-01-10
Author has **439** answers

Step 1

Given:

Mass of nitrogen =75.2 g (75.2% by mass)

Mass of krypton =24.8 g (24.8% by mass)

Total pressure =745 mm Hg

Step 2

To determine the partial pressure of krypton as follows,

Molar mass of nitrogen =28.02

Calculating the moles of nitrogen using the formula,

=2.68mol

Molar mass of krypton =83.80

Calculating the moles of krypton using the formula,

Mass of krypton

=0.296mol

Step 3

To calculate the mole fraction of krypton,

Moles of krypton,

Partial pressure of krypton =Total pressure * Mole fraction of krypton

Substituting the values in the above formula,

Partial pressure of krypton =745mmHg*0.0995=74.1mmHg

Hence, the partial pressure of krypton in the given mixture is 74.1mmHg .

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