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Dafna11 [192]
3 years ago
13

A gas mixture contains 3.0 mol of hydrogen (H2) and 7.3 mol of nitrogen (N2). The total pressure of the mixture is 304 kPa. What

is the mole fraction and partial pressure of H2?
Chemistry
1 answer:
Inga [223]3 years ago
5 0

Answer:

Mole fraction H₂ = 0.29

Partial pressure of H₂ → 88.5 kPa

Explanation:

You need to know this relation to solve this:

Moles of a gas / Total moles = Partial pressure of the gas / Total pressure

Total moles = 3 mol + 7.3 mol → 10.3 moles

Mole fraction H₂ → 3 moles / 10.3 moles = 0.29

Mole fraction = Partial pressure of the gas / Total pressure

0.29 . 304 kPa = Partial pressure of H₂ → 88.5 kPa

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Magnesium metal (0.100 mol) and a volume of aqueous hydrochloric acid that contains 0.500 mol of HCl are combined and react to c
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2.24 L of hydrogen gas, measured at STP, are produced.

Explanation:

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Moles of hydrochloric acid, HCl = 0.500 mol

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Mg_{(s)} + 2HCl_{(aq)}\rightarrow MgCl_2_{(aq)} + H_2_{(g)}

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1 mole of Mg on reaction forms 1 mole of H_2

0.100 mole of Mg on reaction forms 0.100 mole of H_2

Mole of H_2 = 0.100 mol

At STP,  

Pressure = 1 atm  

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Volume = ?

Using ideal gas equation as:

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Applying the equation as:

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<u>⇒V = 2.24 L</u>

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When a molecule is excited to a higher state it often ends up in its lowest excited state S1 and then emits radiation.

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