The pressure in atmospheres of the given mole and volume of helium gas is 4.7atm.
Given the data in the question;
Pressure in atmosphere; [tex]P = \ ?[/tex]
The Ideal gas law emphasizes on the behavior of a hypothetical ideal gas. It states that pressure P multiply by volume V is equal to moles times temperature and the universal gas constant.
It is expressed;
[tex]PV = nRT[/tex]
Where P is pressure, V is volume, n is the amount of substance, T is temperature and R is the ideal gas constant.( [tex]R = 0.08206Latm/molK[/tex] ).
To determine the pressure in atmosphere, we substitute our values into the expression above.
[tex]PV = nRT\\\\P = \frac{nRT}{V} \\\\P = \frac{1.92mol\ *\ 0.08206Latm/molK\ *\ 298.15K}{10.0L} \\\\P = \frac{46.975Latm}{10.0L}\\\\P = 4.7atm[/tex]
Therefore, the pressure in atmospheres of the given mole and volume of helium gas is 4.7atm.
Learn more about Ideal Gas Law: brainly.com/question/4147359
