Answer:
0.558 atm
Explanation:
We must first consider that both gases behaves like ideal gases, so we can use the following formula: PV=nRT
Then, we should consider that, whithin a mixture of gases, the total pressure is the sum of the partial pressure of each gas:
P₀ = P₁ + P₂ + ....
P₀= total pressure
P₁=P₂= is the partial pressure of each gass
If we can consider that each gas is an ideal gas, then:
P₀= (nRT/V)₁ + (nRT/V)₂ +..
Considering the molecular mass of O₂:
M O₂= 32 g/mol
And also:
R= ideal gas constant= 0.082 Lt*atm/K*mol
T= 65°C=338 K
4.98 g O₂ = 0.156 moles O₂
V= 7.75 Lt
Then:
P°O₂=partial pressure of oxygen gas= (0.156x0.082x338)/7.75
P°O₂= 0.558 atm
<span>A) indicate the general distribution of electrons among bonded atoms in molecular compounds
B)</span>useful in naming compounds, writing formulas, and balancing chemical equations
<span>may be used to determine the simplest chemical formula </span>
The mass of the ball is 1.55 kg and its change in momentum is 10 kgm/s.
<h3>What is momentum of a body?</h3>
The momentum of a body is the product of the mass and velocity of the body.
- Momentum = mass * velocity
Mass of the ball = momentum/velocity
Mass of the ball = 3.29 / 2.11 = 1.55 kg
The change in momentum of the body or Impulse = force * time
Change in momentum of the body = 5.00 * 2.00 = 10 kgm/s
Therefore, the momentum of a body depends on its mass and velocity.
Learn more about momentum at: brainly.com/question/1042017
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