Answer:
1.91 atm
Explanation:
Step 1: Calculate Henry's constant (k)
A gas has a solubility (C) of 2.45 g/L at a pressure (P) of 0.750 atm. These two variables are related to each other through Henry's law.
C = k × P
K = C/P
K = (2.45 g/L)/0.750 atm = 3.27 g/L.atm
Step 2: Calculate the pressure required to produce an aqueous solution containing 6.25 g/L of this gas at constant temperature.
We have C = 6.25 g/L and k = 3.27 g/L.atm. The required pressure is:
C = k × P
P = C/k
P = (6.25 g/L)/(3.27 g/L.atm) = 1.91 atm
Answer:
Percent yield = 82.5
Explanation:
Given data:
Actual yield of N₂ = 275 L
Theoretical yield = 333 L
Percent yield = ?
Solution:
Chemical equation:
4HCl + 6NO → 5N₂ + 6H₂O
Percent yield:
Percent yield = actual yield / theoretical yield × 100
Percent yield = (275 L/ 333 L ) × 100
Percent yield = 0.825× 100
Percent yield = 82.5%
Answer : The mass of 
dissolved will be, 0.2365 grams
Explanation :
First we have to calculate the concentration of .
As we know that,
where,
= concentration of = ?
= partial pressure of = 1.65 atm
= Henry's law constant = 
Now put all the given values in the above formula, we get:
The concentration of = 
Now we have to calculate the moles of
Now we have to calculate the mass of
Therefore, the mass of dissolved will be, 0.2365 grams
Answer:
They are directly proportional
Explanation:
when the kelvin temperature increases, the average kinetic energy of particles increases and they move faster and vice versa.
