If I have 0.725 moles of gas at a temperature of 105 K and a pressure of 3.75 atmospheres, what is the volume of the gas?
1 answer:
If I have 0.725 moles of gas at a temperature of 105 K and a pressure of 3.75 atmospheres the volume of the gas 1.66 litres.
Explanation:
Data given:
number of moles of the gas = 0.725
temperature = 105 K
pressure = 3.75 atm
volume of the gas =?
R = 0.08206 Latm/mole Kelvin
Applying the ideal gas law to calculate the volume of the given gas:
PV = nRT
rearranging the equation to calculate volume:
V =
putting the values in the equation:
V =
V = 1.66 Litres.
At a temperature of 105 K and pressure of 3.75 atm, 0.725 moles of gas occupy 1.66 litres of volume.
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Answer:
See detailed mechanism in the image attached
Explanation:
The mechanism shown in detail below is the synthesis of serine in steps.
The first step is the attack of the ethoxide ion base on the diethyl acetamidomalonate substrate giving the enolate and formaldehyde.
The second step is the protonation of the oxyanion from (1) above to form an alcohol as shown.
Acid hydrolysis of the alcohol formed in (3) above yields a tetrahedral intermediate, a dicarboxyamino alcohol.
Decarboxylation of this dicarboxyamino alcohol yields serine, the final product as shown in the image attached.
