Ideal gases are often studied at standard ambient temperature and pressure (satp). The international union of pure and applied c
1 answer:
This problem provides information about the pressure and temperature ideal gases are studied at. The answer to the questions are that all molecules have the same density, 2.43x10²⁵ mol/m³ and 2.43x10¹⁹ mol/cm³.
<h3>Idela gases</h3>In science, we can start studying gases with the concept of ideal gas, as they do not collide one to another and are assumed to be perfect spheres with no relevant interactions.
In such a way, one can conclude that the <u>number density of all ideal gasses at SATP is the same</u>, as they are assumed to be perfect spheres with equal volumes per molecule.
Moreover, when calculating the number of molecules per cubic meter, one must use the ideal gas equation as:
And plug in the numbers we are given:
Lastly, we can calculate the molecules per cubic centimeter by performing the following conversion:
Learn more about ideal gases: brainly.com/question/26450101
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The figure shown below illustrates a lever being used to lift a weight W.
The applied force is F.
In order to lift the weight, the minimum applied force is
F*b = W*a
F = (a/b)W
When the ratio a/b < 1, then the applied force is less than the weight.
The principle behind the use of a lever is to keep the ratio a/b small in order to decrease the effort force.
Answer: A
A lever is used to decrease effort force.
The applied force is F.
In order to lift the weight, the minimum applied force is
F*b = W*a
F = (a/b)W
When the ratio a/b < 1, then the applied force is less than the weight.
The principle behind the use of a lever is to keep the ratio a/b small in order to decrease the effort force.
Answer: A
A lever is used to decrease effort force.
To solve the problem, we can use Charle's law, which states that for an ideal gas at constant pressure the ratio between absolute temperature T and volume V remains constant:
For a gas transformation, this law can be rewritten as
(1)
where 1 and 2 label the initial and final conditions of the gas.
Before applying the law, we must convert the temperatures in Kelvin:
The initial volume of the gas is
, so if we re-arrange (1) we find the new volume of the gas:
For a gas transformation, this law can be rewritten as
where 1 and 2 label the initial and final conditions of the gas.
Before applying the law, we must convert the temperatures in Kelvin:
The initial volume of the gas is