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Ray Of Light [21]
3 years ago
6

The pressure of a gas is caused by

Chemistry
2 answers:
katen-ka-za [31]3 years ago
6 0

The rapid motion and collisions of molecules with the walls of the container causes pressure.

Marrrta [24]3 years ago
4 0

Answer:

The rapid motion and collisions of molecules with the walls of the container causes pressure (force on a unit area). Pressure is proportional to the number of molecular collisions and the force of the collisions in a particular area. The more collisions of gas molecules with the walls, the higher the pressure.

(Don't know for sure but...)

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Match each term to its description.
stepladder [879]

Based on ecological studies, the definitions below applies to the given terms:

  • Peak phenomena: this is when a population grows at a fast rate, then quickly drops when the resources run out
  • Biological surplus: this occurs when there are more organisms in a population than the ecosystem can sustain
  • Climax community: this is a point in an ecosystem when all populations reach a point of little or no change
  • Sigmoid phenomena: this is when a population increases while food and habitat are abundant and decreases as food becomes less available

<h3>What is ecology and what are some terms in ecology?</h3>

Ecology is the study of living things and their interactions with their environment.

Some terms in ecology include:

  • Peak phenomena: this is when a population grows at a fast rate, then quickly drops when the resources run out
  • Biological surplus: this occurs when there are more organisms in a population than the ecosystem can sustain
  • Climax community: this is a point in an ecosystem when all populations reach a point of little or no change
  • Sigmoid phenomena: this is when a population increases while food and habitat are abundant and decreases as food becomes less available

Learn more about Peak phenomena, Biological surplus, Climax community and Sigmoid phenomena at: brainly.com/question/7149100

8 0
2 years ago
Which condition increases the number of collisions between reactant molecules in a given volume?
Nezavi [6.7K]

Answer:

Increasing Surface Area

Explanation:

A greater surface area (meaning more, smaller particles) allows for more opportunity for particles to collide.  On the other hand, decreasing temperature and removing a catalyst would only decrease the number of collisions, and the clumping option doesn't make much sense.  Hope this helps!

4 0
3 years ago
Read 2 more answers
1. What kind of diagram shows how energy flows from one organism to another?
shusha [124]
It would be D.the food chain
5 0
2 years ago
A sample of air was collected on a day when the total atmosphere pressure was
zhuklara [117]

Answer:

1. The gas law used: Dalton's law of partial pressure.

2. Pressure of nitrogen = 331 mmHg

Explanation:

From the question given above, the following data were obtained:

Total pressure (Pₜ) = 592 mmHg

Pressure of Oxygen (Pₒ) = 261 mmHg

Pressure of nitrogen (Pₙ) =?

The pressure of nitrogen in the sample can be obtained by using the Dalton's law of partial pressure. This is illustrated below:

Pₜ = Pₒ + Pₙ

592 = 261 + Pₙ

Collect like terms

592 – 261 = Pₙ

331 = Pₙ

Pₙ = 331 mmHg

Therefore, the pressure of nitrogen in the sample is 331 mmHg

5 0
2 years ago
If a car can go from 0 to 60 mi/hr in 8.0 seconds, what would be its final speed after 5.0 seconds if its starting speed were 50
tangare [24]

Answer:

87.5 mi/hr

Explanation:

Because a = Δv / Δt (a = vf - vi/ Δt), we need to find the acceleration first to know the change in velocity so we can determine the final velocity.

vf = 60 mi/hr

vi = 0 mi/hr

Δt = 8 secs

a = vf - vi/ Δt

= 60 mi/hr - 0 mi/hr/ 8 secs

= 60 mi/hr / 8 secs

= 7.5 mi/hr^2

Now that we know the acceleration of the car is 7. 5 mi/hr^2, we can substitute it in the acceleration formula to find the final velocity when the initial velocity is 50 mi/hr after 5 secs.

vi = 50 mi/ hr

Δt = 5 secs

a = 7.5 mi/ hr^2

a = vf - vi/ Δt

7.5 = vf - 50 mi/hr / 5 secs

37.5 = vf - 50

87.5 mi/ hr = vf

7 0
3 years ago
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