2. Which statement is true regarding the motion of liquid water molecules and ice molecules?
1 answer:
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<h2>Answer:</h2>
44.06 g/mol
<h3>Explanation:</h3>We are given;
- Number of moles of unidentified gas as 1.674×10^-4 mol
- Time of effusion of unidentified gas 86.6 s
- Number of moles of Argon gas as 1.715×10^-4 mol
- Time of effusion of Argon gas is 84.5 s
We are supposed to calculate the molar mass of unidentified gas
<h3>Step 1: Calculate the effusion rates of each gas</h3>Effusion rate = Number of moles/time
Effusion rate of unidentified gas (R₁)
= 1.674×10^-4 mol ÷ 86.6 s
= 1.933 × 10^-6 mol/s
Effusion rate of Argon gas (R₂)
= 1.715×10^-4 mol ÷ 84.5 sec
= 2.030 × 10^-6 mol/s
<h3>Step 2: Calculate the molar mass of unidentified gas</h3>- Assuming the molar mass of unidentified gas is x;
- We can use the Graham's law of effusion to find x;
- According to Graham's law of diffusion;
But, Molar mass of Argon is 39.948 g/mol
Therefore;
Solving for X
x = 44.06 g/mol
Therefore, the molar mass of the identified gas is 44.06 g/mol
Answer:
8.55 moles
Explanation:
The formula for calculating molarity is moles of solute divided by liters of solution. In this case:
moles. Hope this helps!