Question

calculate the no of molecules present in 2.5 litre of co2 measured at 27° and 744 mm hg pressure​

Answer 1

Answer:

Hope this is correct answer

Explanation:

Here, T=27

∘

C=27+273=300K

P=2.5 atm

The molar mass of(M) CO

2

=44g/mol

From ideal gas equation,

d=

RT

PM

=

0.0821×300

2.5×44

=4.46 g L

−1

Answer 2

Answer:

The no.of molecules in the given gas are $5.97\times10^{22}$ molecules

Explanation:

Given that,

The volume of the carbon dioxide is $V=2.5L$

The temperature of the gas is $T=27+273=300K$

And the pressure is given as $P=744mm of hg=0.978atm$

We are required to find the no.of molecules present in the gas.For that we use the ideal gas equation which is shown below

$PV=nRT$

Here R is the universal gas constant and its value is $R=0.0821L.atm/K/mol$

Substituting the values of pressure,volume,temperature and gas constant in the above relation we get-

$0.978\times2.5=n\times0.0821\times300\\= > n=\frac{2.445}{24.63} =0.099 mol$

As the number of moles are obtained,we shall multiply it with Avagadro number to obtain no.of molecules.We do is as shown below-

$=0.099\times6.023\times10^{23}=5.97\times10^{22}$

Therefore,the number of molecules in the given gas are $5.97\times10^{22}$ molecules.

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