Question

0.7 g of a gas at STP occupies a volume of 0.56 L, the gas can be

Answer 1

Explanation:

pv=NRT

so here P=1 at stp

V=0.56

N= 0.7/x

R=0.08

T=273

on applying this in equation we get

1×0.56=0.7/x×0.08×273

where x is the molar mass

solving we get x= 28( approx)

so CO will be the correct answer

Answer 2

Given: $0.7$ g of a gas at STP occupies a volume of $0.56$ L.

We have to find the type of gas.

The given problem is solved in the following way,

As we know that one mole of gas at STP occupies $22.4$liters.

Therefore,

$=>\frac{0.56}{22.4} \\=>0.025$

Thus, $0.56$ liters of gas at STP contain $0.025$moles.

We know that,

$\text { no.ofmoles }=\frac{\text { wt.ingrams }}{\text { Mol.wt. }}\\\\=>0.025=\frac{0.7}{M.wt.}\\\\=>M=28$

Nitrogen gas has a molecular weight$28$.

Therefore the gas will be Nitrogen.