Each of the following flasks have the same number of gas molecules at same tempe

Question

Each of the following flasks have the same number of gas molecules at same temperature. Which flask will have the greatest pressure? A student collects 425 mL of oxygen gas at a temperature of 24 degree C and a pressure of 0.899 atm. How many grams of oxygen gas did the student collect? A bulb with a volume of 225 mL contains 0.580 g of an unknown gaseous compound. The pressure is measured at 145.60 kPa at a temperature of 25 degree C. What is the molar mass of the compound? Determine the density of nitrogen gas at 3.10 atm and -5.0 degree C. How many grams of water would be produced if 20.0 liters of oxygen were burned at a temperature of-10.0 degree C and a pressure of 1.3 atm? 2 C_8H_18(I) + 25 O_2 (g) 16 CO_2 (g) + 18 H_20 (g) Use the chemical equation from #67. If you burned one gallon of gas(C_8H_18) (approximately 4000. grams), how many liters of carbon dioxide would be produced at a temperature of 21.0 degree C and a pressure of 1.00 atm?

Explanation / Answer

63)
since number of moles and temperature is same,
P and V will be inversely proportional according to Boyle's law

smaller the volume, greater will be the pressure

Answer: Flask 1 will have greatest pressure

64)
1st find number of moles of O2 gas using,
P*V = n*R*T
0.899 atm * 0.425 L = n*0.0821 atm.L/mol.K * (24 + 273) K
0.899*0.425 = n * 0.0821*297
n = 0.1567 mol

molar mass of O2 = 32 g/mol

mass of O2 = number of moles * molar mass
= 0.1567 mol * 32 g/mol
= 0.50 g

Answer: 0.50 g

I am allowed to answer only 1 question at a time

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