A sample of an ideal gas has a volume of 2.31 l at 287 k and 1.10 atm. calculate the pressure when the volume is 1.45 l and the
1 answer:
Hello!
The pressure of the Ideal Gas when the volume is 1,45 L and the temperature is 298 K is 1,82 atm.
To solve this problem we need to apply the Ideal Gas Law for the initial conditions and the final ones, clearing the equation for the number of moles (n) and the ideal gas constant (R) which remain constant:
Now we match n*R for the initial conditions (1) and the final ones (2), clearing the equation for P₂
Have a nice day!
The pressure of the Ideal Gas when the volume is 1,45 L and the temperature is 298 K is 1,82 atm.
To solve this problem we need to apply the Ideal Gas Law for the initial conditions and the final ones, clearing the equation for the number of moles (n) and the ideal gas constant (R) which remain constant:
Now we match n*R for the initial conditions (1) and the final ones (2), clearing the equation for P₂
Have a nice day!
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Both aluminum and chlorine have known charges, which are +3 and -1 respectively. To make them cancel each other out in charge, you would need 3 chlorine and for one aluminum, therefore 
would be correct
Answer:
A, C and D are correct.
Explanation:
Hello.
In this case, since the relationship between the vapor pressure of a solution is directly proportional to the mole fraction of the solvent and the vapor pressure of the pure solvent as stated by the Raoult's law:
Since the solute is not volatile, the mole fraction of the solute is not taken into account for vapor pressure of the solution, therefore A is correct whereas B is incorrect.
Moreover, since the higher the vapor pressure, the weaker the intermolecular forces due to the fact that less more molecules are like to change from liquid to vapor and therefore more energy is required for such change, we can evidence that both C and D are correct.
Best regards.