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Genrish500 [490]
3 years ago
14

Compute the specific heat capacity at constant volume of nitrogen (N2) gas. The molar mass of N2 is 28.0 g/mol.

Chemistry
1 answer:
goldfiish [28.3K]3 years ago
8 0

Answer:Specific heat capacity at Constant volume of Nitrogen =742.32JKg.K

Explanation:

The Specific heat capacity at Constant volume of an ideal gas is given as

c =Cv / M

Cv= Constant volue of gas

M= Molar mass

But  First, we determine the Constant volume, Cv  which is given as

Cv = 5/2R since Nitrogen is a diatomic gas, N2 where R= 8.314Jmol.k

= 5/2 x 8.314Jmol.K

=20.785Jmol.K

Specific heat capacity at Constant volume, c

c= Cv/M

M=molar mass = 28.0 g/mol.

changing to kg/mol =28/1000= 0.028kg/mol

Therefore c =20.785Jmol.K/0.028kg/mol

=742.32JKg.K

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P₂ ≅ 100 atm (1 sig. fig. based on the given value of P₁ = 90 atm)

Explanation:

Given:

P₁ = 90 atm                    P₂ = ?

V₁ = 18 Liters(L)              L₂ = 12 Liters(L)      

=> decrease volume => increase pressure

=> volume ratio that will increase 90 atm is (18L/12L)                                                                  

T₁ = 272 Kelvin(K)          T₂ = 274 Kelvin(K)

=>  increase temperature => increase pressure

=> temperature ratio that will increase 90 atm is (274K/272K)

n₁ = moles = constant    n₂ = n₁ = constant

P₂ = 90 atm x (18L/12L) x (274K/272K) = 135.9926471 atm (calculator)

By rule of sig. figs., the final answer should be rounded to an accuracy equal to the 'measured' data value having the least number of sig. figs. This means P₂ ≅ 100 atm based on the given value of P₁ = 90 atm.

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