Answer:
0.7atm
Explanation:
Given parameters:
Initial temperature = 25.2°C in Kelvin; 25.2 + 273 = 298.2K
Initial pressure = 0.6atm
Final temperature = 72.4°C in kelvin = 72.4 + 273 = 345.4K
Unknown:
Final pressure = ?
Solution:
Since we are dealing with pressure temperature relationships under a fixed volume, we use a simplification of the combined gas law to solve this problem.
At fixed volume;
where P and T are temperature values
1 and 2 are the initial and final states
Input the parameters and solve for P₂
P₂ = 0.7atm
The freezing point depression is a colligative property, which means that it depends on the number of particles of solute disolved in the solution.
When you have solutes that are ionic compounds they dissociate in water into ions, then the compound that dissociates more ions will produce more particles and will decrease the freezing point the most.
Given theses aqueous solutions Na2 CO3, Co Cl3, and Li NO3 you can predict the order of the freezing points.
First, write the dissociation equations>
Na2CO3 -> 2Na(+) + CO3 (2-) These are 3 ions: two of Na(+) and one of CO3(2-)
The number inside parenthesis are number of charge not number of molecules.
Co Cl3 -> Co(3+) + 3 Cl (1-) Those are 4 ions: one of Co (+) and three of Cl (-)
Li NO3 -> Li (+) + NO3 (-) those are two ions: one of Li (+) and one of NO3(-)
Then the ionic compound that dissociates into more ions give the solution with lower freezing point, and these is the rank from higher to lower freezing point:
Li NO3 > Na2 CO3 > Co Cl3.
First, we assume that helium behaves as an ideal gas such that the ideal gas law is applicable.
PV = nRT
where P is pressure, V is volume, n is number of moles, R is universal gas constant, and T is temperature. From the equation, if n, R, and T are constant, there is an inverse relationship between P and V. From the given choices, the container with the greatest pressure would be the 50 mL.
Answer:
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Explanation:
