A volume of 10.0L of gas at a temperature of 5c is cooled to a temperature of 85C at constant pressure what is the new volume of
gas
2 answers:
Answer:
At constant pressure the new volume of gas is 12.878 L.
Explanation:
Charles's Law consists of the relationship between the volume and temperature of a certain amount of ideal gas, which is maintained at a constant pressure, by means of a proportionality constant that is applied directly. So the ratio between volume and temperature will always have the same value:
where the temperature is expressed in degrees kelvin (° K)
Then, when considering the two situations 1 and 2, keeping the amount of gas and the temperature constant, the relationship must be met:
In this case, you know:
- V1= 10 L
- T1= 5 +273 = 278°K (where 0°C=273°K)
- V2= ?
- T2= 85 + 273 = 358°K
Replacing:
Solving:
V2=12.878 L
<u><em>At constant pressure the new volume of gas is 12.878 L.</em></u>
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Answer:
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Explanation:
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The mechanism is taking place in 3 steps.
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The second step involves the breaking of this bond to have the OMgBr and the propyl attached to the carbon of the chain.
The last steps involves an hydration of the molecule, to turn the OMgBr into OH, and that would be the final product.
In this case, the final product will be 1-propyl-cyclohexanol.
The picture below, shows the mechanism and the drawing of the final product.
