Answer:
5.7 grams is the mass carbon dioxide gas inside a 3.0-L balloon.
Explanation:
Using ideal gas equation:
PV = nRT
where,
P = Pressure of carbon dioxide gas =
V = Volume of carbon dioxide gas = 3.0 L
n = number of moles of carbon dioxide gas = ?
R = Gas constant = 0.0821 L.atm/mol.K
T = Temperature of carbon dioxide gas =0°C = 0+273= 273 K
Putting values in above equation, we get:
Mass of 0.13 mole carbon dioxide gas :
= 0.13 mol × 44 g/mol = 5.7 g
5.7 grams is the mass carbon dioxide gas inside a 3.0-L balloon.
Answer:
Explanation:
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In this case, since the undergoing chemical reaction is:
It is widely known that when a gas given off from a reaction is collected over water, we can compute its pressure by minusing the total pressure 762 mmHg and the vapor pressure of water at the experiment's temperature (20 °C) in this case 17.5 mmHg as shown below:
Next, by using the ideal gas equation we compute the yielded moles of oxygen considering the collected 313 mL (0.313 L):
Now, via the 3/2:1 mole ratio between oxygen and lithium chlorate (molar mass = 90.39 g/mol), we compute the original mass of decomposed lithium chlorate as follows:
Now, the percentage is computed as shown below:
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