Question

question 5 (2 points)
the total pressure in a container is 25.0 atm. it contains 50.0% oxygen, 45.0%
nitrogen, and the rest is hydrogen. what is the partial pressure of the hydrogen?
this is a 1 type of problem so we use the equation 2.
the container is 5.00% hydrogen, thus 5.00% of the 25.0 atm is from hydrogen. this
corresponds to (0.0500)(25.0 atm) = 3 atm
a. missing variable b. change in conditions c. density d. molar volume at stp
e. partial pressure f. 1 mol = 22.4 l g. d = m/v h. pv = nrt
i. p2v2/n2t2 = p1v1/n1t1 j. ptotal = p1 + p2 + …… k. p l p1 m. p2
n. v o. v1 p. v2 q. n r. n1 s. n2 t. r u. t
v. t1 w. t2 x. 1.25 y. 12.5 z. 125

Explanation:

Step1: Determine the type of problem

The problem is about partial pressure as we are dealing with the pressure of a component (hydrogen) in a mixture of gases.

Step2: Identify the relevant equation

For partial pressure in a gas mixture, the equation \(P_{total}=P_1 + P_2+\cdots\) (where each \(P_i\) is the partial pressure of a gas component) is relevant. But when we know the mole - fraction (or in this case, percentage by volume which is equivalent to mole - fraction for ideal gases) of a gas, we can use \(P_i = X_iP_{total}\) (where \(X_i\) is the mole - fraction of gas \(i\)). Here, since the percentage of hydrogen is given, we can directly calculate its partial pressure using \(P_{H_2}=X_{H_2}P_{total}\)

Step3: Calculate the partial pressure of hydrogen

Given \(X_{H_2}=0.0500\) and \(P_{total} = 25.0\ atm\). Then \(P_{H_2}=(0.0500)\times(25.0\ atm)=1.25\ atm\)

Answer:

1. E. partial pressure
2. \(P_i = X_iP_{total}\) (or conceptually related to \(P_{total}=P_1 + P_2+\cdots\) as we are finding one of the \(P_i\) values)
3. X. 1.25