Question

calculate the pressure exerted by 8.5 g of NH3 contained in 0.5 l vessel at 300 K . For NH3...​

Answer 1

$\;\;\;\;\;\;\;\;\;\;\;\;\;⋆\;{\underline{\boxed{\bf{\frak{\pink{\; Given :}}}}}}\;\star$

Mass of ammonia = 8.5 g

Volume of container = 0.5 L

Temperature = 300 K

$\;\;\;\;\;\;\;\;\;\;\;\;\;⋆\;{\underline{\boxed{\bf{\frak{\red{\; To~ Find :}}}}}}\;\star$

Pressure exerted by ammonia gas.

$\;\;\;\;\;\;\;\;\;\;\;\;\;⋆\;{\underline{\boxed{\bf{\frak{\blue{\; Solution :\;}}}}}}\;\star$

✬ First of all we have to find moles of ammonia.

It is defined as the ratio of mass to the molar mass.

Moral mass of NH₃ = 17 g/mol

➙ n = W / Mw

➙ n = 8.5 / 17

➙ n = 0.5

Ideal gas equation is given by

$\dag\:\underline{\boxed{\bf{\green{PV = nRT}}}}$

• P denotes pressure
• V denotes volume
• n denotes number of moles
• R denotes gas constant
• T denotes temperature

By substituting the given values;

: ⟼ PV = nRT

: ⟼ P × 0.5 = 0.5 × 0.082 × 300

: ⟼ P = 0.082 × 300

: ⟼ $\dag\:\underline{\boxed{\bf{\purple{P = 24.6 atm}}}}$

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Hope it's helpful :)

Answer 2

Mass of ammonia = 8.5 g

Volume of container = 0.5 L

Temperature = 300 K

\;\;\;\;\;\;\;\;\;\;\;\;\;⋆\;{\underline{\boxed{\bf{\frak{\red{\; To~ Find :}}}}}}\;\star⋆

To Find:

⋆

Pressure exerted by ammonia gas.

\;\;\;\;\;\;\;\;\;\;\;\;\;⋆\;{\underline{\boxed{\bf{\frak{\blue{\; Solution :\;}}}}}}\;\star⋆

Solution:

⋆

✬ First of all we have to find moles of ammonia.

It is defined as the ratio of mass to the molar mass.

Moral mass of NH₃ = 17 g/mol

➙ n = W / Mw

➙ n = 8.5 / 17

➙ n = 0.5

Ideal gas equation is given by

\dag\:\underline{\boxed{\bf{\green{PV = nRT}}}}†

PV=nRT

P denotes pressure

V denotes volume

n denotes number of moles

R denotes gas constant

T denotes temperature

By substituting the given values;

: ⟼ PV = nRT

: ⟼ P × 0.5 = 0.5 × 0.082 × 300

: ⟼ P = 0.082 × 300

: ⟼ \dag\:\underline{\boxed{\bf{\purple{P = 24.6 atm}}}}†

P=24.6atm

________________________

Hope it's helpful :)