If 1.08 g of sodium sulfate reacts with an excess of phosphoric acid, how much sulfuric acid is produced? Show all work. PLEASE
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Answer:
11.94 grams of carbon dioxide were originally present.
19.94 grams of krypton can you recover.
Explanation:
Mass of carbon dioxide gas = x
Mass of krypton gas = y
x + y = 31.7 g
Moles of carbon dioxide gas =
Moles of krypton gas =
Mole fraction of krpton =
Total pressure of the mixture = P = 0.665 atm
Partial pressure of carbon dioxide gas = p
Partial pressure of krypton gas before removal of carbon dioxide gas = p'
Partial pressure of krypton gas after removal of carbon dioxide gas = p'' = 0.309 atm
p' = p'' = 0.309 atm
0.665 atm = p + 0.309 atm
p = 0.665 atm - 0.306 atm = 0.359 atm
Partial pressure of krypton can also be given by :
..[2]
Solving [1] and [2]:
x = 11.94 g
y = 19.76 g
11.94 grams of carbon dioxide were originally present.
19.94 grams of krypton can you recover.
<u>Answer:</u> The temperature of the ideal gas is
<u>Explanation:</u>
To calculate the temperature, we use the equation given by ideal gas equation:
where,
P = Pressure of the gas = 142,868 Pa = 142.868 kPa (Conversion factor: 1 kPa = 1000 Pa)
V = Volume of gas = 1.0000 L
n = number of moles of ideal gas = 0.0625 moles
R = Gas constant =
T = temperature of the gas = ?
Putting values in above equation, we get:
Hence, the temperature of the ideal gas is