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The false statement from the above is that: Temporary charge imbalances in the molecules lead to London dispersion forces.
<h3>What are the factors that affect London dispersion forces?</h3>
Generally, the factors which affects the London dispersion forces a dispersion force are as follows:
- Shape of the molecules
- Distance between molecules
- Polarizability of the molecules
However, London dispersion forces simply refers to a sort of temporary attractive force formed when electrons in two adjacent atoms occupy positions that make the atoms form dipoles.
So therefore, temporary charge imbalances in the molecules lead to London dispersion forces is a false statement
Learn more about London dispersion forces:
brainly.com/question/1454795
Answer:
In the kinetic molecular theory, the molecules of an ideal gas are in constant random motion inside the container of the gas, and the pressure of the gas (which is the pressure exerted by the molecules in their collisions with the walls of the container) arise from this random motion of the molecules.
The main assumptions of the kinetic theory of gases are:
- The gas consists of a large number of molecules that collide between each other and the walls of the container; all these collisions are elastic
- The duration of the collisions is negligible compared to the time between the collisions
- The number of molecules is so large that statistics can be applied
- Intermolecular forces between the molecules are negligible (except during the collisions)
- The volume of the molecules is negligible compared to the volume of the container
In particular, the pressure of the gas is directly proportional to the average kinetic energy of the molecules, according to the equation:
where
p is the pressure of the gas
V is the volume of the container
K is the average kinetic energy of the molecules in the gas
We see that as the pressure is higher, the higher the kinetic energy of the particles: this means that the molecules will move faster, on average.
Therefore in this problem, the gas that exerts a pressure of 1.5 atm will have molecules moving faster than the molecules of the gas exerting a pressure of only 1.0 atm.
<span>A reversible reaction is a chemical change in which the products can be converted back to the original reactants under suitable conditions.</span><span> In a reversible reaction, changing the reaction conditions e.g. concentration, pressure or temperature will change the net direction the reaction goes i.e. more to the right (forward) or more to left (backward).<span>It also means a reversible reaction does not go to completion in either direction and all components, original reactants or ensuing products, ALL co-exist in the reaction mixture (see notes on chemical equilibrium).</span></span><span><span>This means the reaction can go in either direction i.e.</span><span> <span>A + B ==> C + D or C + D ==> A + B</span></span></span><span><span>A reversible reaction is shown by the sign ,</span><span> <span>a half-arrow to the right (direction of forward reaction), </span><span>and a half-arrow to the left (direction of backward reaction).</span><span>It is really important you understand that the terms right & left AND forward & backward are used in the context of how the equation is presented.</span></span></span><span><span>Most reactions are not reversible (irreversible) and have the usual complete arrow only pointing to the right.</span>
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Answer:
independant=variable that has changed
dependant=variable affected by the change
water=independant, because if you put too much water the dependant that depends on water could die or too little dependant can die (dependant=plants)
Explanation:
