Question

a container has 64 grams of O2 at temperature t and pressure p if same container has 88 grams of H2 at temperature t to then its pressure will be​

Answer 1

pressure of H2 will be 22P

in the same container, pressure of gaseous molecules is directly proportional to number of moles at the same temperature.

i.e., P ∝ n

where P is pressure and n is no of moles.

weight of O2 = 64g

molecular weight of O2 = 32g/mol

so, no of moles of O2 = 64/32 = 2

similarly, weight of H2 = 88g

molecular weight of H2 = 2g/mol

so, no of moles of H2 = 88/2 = 44

now, P1/P2 = n1/n2

⇒P/P2 = 2/44

⇒P/P2 = 1/22

⇒P2 = 22P

so the pressure of H2 at same temperature is 22P

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Answer 2

$\huge\bold\purple{Answer:-}$

in the same container, pressure of gaseous molecules is directly proportional to number of moles at the same temperature.

i.e., P ∝ n

where P is pressure and n is no of moles.

weight of O2 = 64g

molecular weight of O2 = 32g/mol

so, no of moles of O2 = 64/32 = 2

similarly, weight of H2 = 88g

molecular weight of H2 = 2g/mol

so, no of moles of H2 = 88/2 = 44

now, P1/P2 = n1/n2

⇒P/P2 = 2/44

⇒P/P2 = 1/22

⇒P2 = 22P

so the pressure of H2 at same temperature is 22P