If all of the helium was released into a large plastic balloon at a constant tem

Question

If all of the helium was released into a large plastic balloon at a constant temperature and the pressure of the gas drops to 6.00 atm, what would be the volume of the balloon after it expands?

A car tire at has a pressure of 2.5 atm at 30°C. What would the tire pressure be at 20°C, assuming the volume of the tire and the amount of air within stays constant

What isThe release of CO2 from the decomposition of baking soda causes breads to rise the density of oxygen (O2) gas at 25°C and 1 atm

The release of CO2 from the decomposition of baking soda causes breads to rise.
2NaHCO3 (s) Na2CO3(s) + H2O (l) + CO2(g)
If the recipe uses 5.00g of baking soda, what number of moles (n = ?) of CO2 will be formed

If the oven is at 200°C and the pressure is 1 atm, what is the volume of CO2 released?
10. A lab studying air pollution made a mix of 2.00g nitrous oxide (N2O), 3.00g sulfur dioxide (SO2), and 1.00g carbon monoxide (CO) in a sealed container. If the mixture has a pressure of 0.22 atm, what is the partial pressure of sulfur dioxide?

Explanation / Answer

1)

we know that

PV = nRT

given

volume and amount (n) are constant

so

P/T = constant

P1/T1 = P2/T2

given

P1 = 2.5

T1 = 30 + 273 = 303 K

T2 = 20 + 273 = 293 K

so

2.5 / 303 = P2 / 293

P2 = 2.4175

so

pressure in the car tire is 2.4175 atm at 20 C

3)

we know that

moles = mass / molar mass

so

moles of NaHC03 = 5 / 84 = 0.05952381

now

consider the reactin

2NaHC03 ---> Na2C03 + H20 + C02

we can see that

moles of C02 formed = 0.5 x moles of NaHC03 reacted

moles of CO2 formed = 0.5 x 0.05952381

moles of CO2 formed = 0.02976

now

PV = nRT

1 x V = 0.02976 x 0.0821 x 473

V = 1.15575

s

volume of CO2 released is 1.15575 L

10)

we know that

moles = mass / molar mass

so

moles of N20 = 2 / 44 = 0.0454545

moles of S02 = 3 / 64 = 0.046875

moles of C0 = 1 / 28 = 0.0357143

now

total moles= 0.0454545 + 0.046875 + 0.0357143

total moles = 0.1280438

now

mole fraction of S02 = moles of S02 / total moles

mole fraction of S02 = 0.046875 / 0.1280438

mole fraction of S02 = 0.366085

now

pS02 = mol fraction of S02 x total pressure

pS02 = 0.366085 x 0.22

pS02 = 0.0805 atm

so

partial pressure of S02 is 0.0805 atm

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