Since volume and temperature are constant, this means that pressure and <u>number of moles</u> are <u>directly </u>proportional. the sample with the largest <u>number of moles</u> will have the <u>high </u>pressure.
Since, the ideal gas equation is also called ideal gas law. So, according to ideal gas equations,
PV = nRT
- P is pressure of the sample
- T is temperature
- V is volume
- n is the number of moles
- R is universal gas constant
At constant volume and temperature the equation become ,
P ∝ nR
since, R is also constant. So, conclusion of the final equation is
P ∝ n
The number of moles and pressure of the sample is directly proportion. So, on increasing number of moles in the sample , pressure of the sample also increases.
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Hey there!
Molarity = 4.8/850 x 1000 =5.647mol/lit or 5.65M
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Answer:
See explanation
Explanation:
In this case, we have to remember that if we want to remove water from the reaction vessel we have to heat the vessel. So, we can convert the liquid water into <u>gas water</u> and we can remove it from the vessel. In this case, the products of dehydration for both molecules are <u>(E)-4-methylpent-2-ene</u> and <u>cyclohexene</u> with boiling points of <u>59.2 ºC</u> and <u>89 ºC</u> respectively. The boiling point of water is <u>100 ºC</u>, therefore if we heat the vessel the products and water would leave the system, and the products would be lost.
See figure 1
I hope it helps!