1 point A container with nitrogen, oxygen, and hydrogen has a pressure of 10.46
atm. If the pressure of nitrogen is 321 kPa and the pressure of oxygen is
74.0 psi, what is the pressure of hydrogen? *
2.25 atm
18.7 atm
4.90 atm
237 atm

2.25 atm

Explanation:

Given data

Step 1: Convert the pressure of nitrogen to atm

We will use the relationship 1 atm = 101.325 kPa.

Step 2: Convert the pressure of oxygen to atm

We will use the relationship 1 atm = 14.6959 psi.

Step 3: Calculate the partial pressure of hydrogen

The total pressure is the sum of the partial pressures.

P = pN₂ + pO₂ + pH₂

pH₂ = P - pN₂ - pO₂

pH₂ = 10.46 atm - 3.17 atm - 5.04 atm

pH₂ = 2.25 atm

Explanation:

Hello,

IN this case, we can apply the Dalton's law in order to understand the pressure behavior of a mixture as the summation of all the pressures of the compounds in the mixture, in this case, nitrogen, oxygen and hydrogen:

So, since we are asked to compute the pressure of hydrogen, we simply solve for it:

Best regards.

the answer is the first option

explanation:

just googled it m8. not that hard

lol

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.