A sample of nitrogen has a volume of 50.0L at a pressure of 760mmHg. What is the volume of the gas at each of the following pres
1 answer:
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Answer:
The Answer is 2,86 grs Na2CO3
Explanation:
What we have to do is find the mass of Na2CO3 as a pure component or solute. That's because the 11,8 mL are a solution of Na2CO3. This means, the sum between the solute Na2CO3 and water. To find the grams of Na2CO3 as pure component we create a factor series as is shown in the attached file.
Data:
Density of solution (ρ) = 1,10 grs sln Na2CO3/mL sln Na2CO3
Mass Percentage (%) = 22 grs Na2CO3/100 grs sln Na2CO3
The procedure is explained in the attached file
1) 2P
2) Average speed does not change
Explanation:
1)
To solve the first part of the problem, we can use Boyle's Law, which states that:
"For a fixed mass of an ideal gas kept at constant temperature, the pressure of the gas is inversely proportional to its volume"
Mathematically:
where
p is the pressure of the gas
V is its volume
For the Xe gas in this problem we can write
where:
is the initial pressure
is the initial volume
is the final volume
Solving for p2, we find the final pressure:
So, the pressure has doubled.
2)
The average speed of the atoms/molecules in the gas is given by the formula
where
R is the gas constant
T is the absolute temperature (in Kelvin) of the gas
M is the molar mass of the gas
is known as rms speed of the particles in the gas
From the formula, we see that the speed of the atoms in the gas depends only on the temperature of the gas.
In the Xe(g) gas in this problem, the temperature is kept constant; therefore, since nothing changes in the formula, this means that the average speed also does not change.