Question

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Answer 1

Answer:-

option(2)

Explanation:-

From Ideal Gas Equation

$\boxed{\green{\mathsf{PV = nRT }}}$

P - pressure

V - Volume of container/ gas

n - No. of moles of gas

R - Gas constant

T - Temp.

Now,

$\mathsf{PV = nRT }$

As we know

$\boxed{\blue{\mathsf{V = \dfrac{m}{d} }}}$

m - mass of gas

d - density

Hence,

$\implies \mathsf{P \: \dfrac{m}{d}= nRT }$

$\implies \mathsf{m \: \dfrac{P}{d}= nRT }$

$\implies \mathsf{ \dfrac{P}{d}= \dfrac{nR(293)}{m} }$

$\implies \mathsf{ \: \dfrac{d}{P}= \dfrac{m}{nR (293)} = k}$ ----(1)

Now,

at 120° C (393k)

$\implies \mathsf{ \: \dfrac{d}{P}= \dfrac{m}{nR (393)} = k' }$ ---(2)

Now

eq. (1) divided by (2)

$\implies \mathsf{ \: \dfrac{k}{k'}= \dfrac{393}{ 293} }$

$\implies \mathsf{ k'= \dfrac{293}{393} \: k }$