Four gases were combined in a gas cylinder with these partial pressures: 3.5 atm N2, 2.8 atm O2, 0.25 atm Ar, and 0.15 atm He. What is the total pressure inside the cylinder? P_(T)=P_(1)+P_(2)+P_(3)+ldots +P_(n) (P_(a))/(P_(T))=(n_(a))/(n_(T)) square Iatm DONE V

To find the total pressure inside the cylinder, we can use Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gases.<br /><br />Given:<br />Partial pressure of N2, $P_{N2} = 3.5$ atm<br />Partial pressure of O2, $P_{O2} = 2.8$ atm<br />Partial pressure of Ar, $P_{Ar} = 0.25$ atm<br />Partial pressure of He, $P_{He} = 0.15$ atm<br /><br />Using Dalton's Law of Partial Pressures:<br />$P_{T} = P_{N2} + P_{O2} + P_{Ar} + P_{He}$<br />$P_{T} = 3.5 + 2.8 + 0.25 + 0.15$<br />$P_{T} = 6.7$ atm<br /><br />Therefore, the total pressure inside the cylinder is 6.7 atm.