Why are water molecules polar? select one:
1 answer:
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The question is incomplete, here is the complete question:
At 25°C Henry's Law constant for carbon dioxide gas in water is 0.031 M/atm . Calculate the mass in grams of gas that can be dissolved in 425. mL of water at 25°C and at a partial pressure of 2.92 atm. Round your answer to 2 significant digits.
<u>Answer:</u> The mass of carbon dioxide that can be dissolved is 1.7 grams
<u>Explanation:</u>
To calculate the molar solubility, we use the equation given by Henry's law, which is:
where,
= Henry's constant =
= molar solubility of carbon dioxide gas
= partial pressure of carbon dioxide gas = 2.92 atm
Putting values in above equation, we get:
To calculate the mass of solute, we use the equation used to calculate the molarity of solution:
Given mass of carbon dioxide = ? g
Molar mass of carbon dioxide = 44 g/mol
Molarity of solution =
Volume of solution = 425 mL
Putting values in above equation, we get:
Hence, the mass of carbon dioxide that can be dissolved is 1.7 grams
Answer:
36.37% is the percent yield of the reaction.
Explanation:
1)0.650 L nitrogen gas , at 295 K and 1.01 bar.
Let the moles of nitrogen gas be n.
Pressure of the gas ,P= 1.01 bar = 0.9967 atm (1 bar = 0.9869 atm)
Temperature of the gas = T = 295 K
Volume of the gas = V = 0.650 L
Using an ideal gas equation:
2) Moles of ammonia gas=
Moles of oxygen gas =
According to reaction ,3 mol of oxygen reacts with 4 mol of ammonia.
Then,0.1101 mol of oxygen will react with:
of ammonia.
Hence, oxygen gas is in limiting amount and act as limiting reagent.
3) Theoretical yield of nitrogen gas :
According to reaction, 3 mol of oxygen gas gives 2 moles of nitrogen gas.
Then 0.1101 mol of oxygen will give:
of nitrogen.
Theoretical yield of nitrogen gas = 0.0734 mol
Experimental yield of nitrogen as calculated in part (1) = 0.0267 mol
Percentage yield:
Percentage yield of the reaction:
36.37% is the percent yield of the reaction.