Answer:
According to the kinetic molecular theory of gases, the average speed and kinetic energy of gas molecules would INCREASE.
Explanation:
In the kinetic molecular theory of gases, assumptions were made based on macroscopic properties of gas (pressure, volume and temperature) which are as a result of the microscopic properties like the position and the speed of the gas molecules. The kinetic molecular theory explains the behaviour of gases through the following 5 assumptions made about an ideal gas;
--> Molecules of a gas are in constant and rapid motion in straight lines until they collide with one another and with the walls of their containers.
--> The actual volume occupied by the had is negligible compared with the volume of the container.
--> Forces of attraction or repulsion between the molecules of a gas are negligible
--> The collision between the molecules is perfectly elastic.
--> The average kinetic energy of the gas molecules is proportional to the temperature of the gas.
Because gas molecules are in constant motion, it has kinetic energy which can be altered when there is increase in pressure. An increase in pressure will cause gas molecules to collide more frequently with one another. This in turn leads to increase in average speed and the kinetic energy of the individual molecules.
Compounds are smaller than atoms is not true
20/32=0.625 moles of sulfur
30/16 = 1.875 moles of oxygen
The formula requires 1 mole of sulfur for 3 moles of oxygen which means that their is no limiting reactant as that is the ratio found thus it will react to completion forming 50 grams of product or sulfur trioxide
Answer:
1. balance observation using "how much" = 5. quantitative instrument
2. graduated cylinder = 4. quantitaive instrument of volume
3. hypothesis proposed explanation= 7. qualitative descriptive observation
4. unit of volume= L
6. kg = primary unit of mass
Explanation:
there seem to be some typo error in uploading question but still it was clear to answer.
The answer is false, oxygen
