Question

If the volume of Nitrogen of mass 14 kg is 0.4 m³ at 30° C; calculate the pressure.

Answer 1

$\huge\pink{As-Salamu-Alykum}$


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$\huge\orange{Given:-}$


Mass=14kg =14000g


Volume = 0.4m^3


Temperature = 30°C


Tk = Tc +273


Tk= 30+273


Tk =303K


Pressure=?


$\huge\orange{Solution:-}$


PV=nRT


n=mass/molar mass


Molar mass of N2 = 28mol


Moles of N2= 14000/28


Moles of N2=500mol


P = nRT/V


R = 0.082litre atom mol^_1K^_1


P = 500 × 0.082 × 303/0.4


P=12423/0.4


P = 31057.5 atm

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Answer 2

Answer:

pressure (P) = 31057.5 atm

Explanation:

as know the formula

PV = nRT==>(1)

here,

Pressure (p) = we need to find.

volume (v) = 0.4 m^3

temperature (T) = 30°C = 303k

no.of moles(n) = wt /gmwt = 14000/28 = 500

gas constant (R) = 0.821

From (1):

P= 500×0.821×303/0.4

therefore, P = 31057.5 atm.....