Question

Pt. A: How many moles of methane gas, CH4, are in a 1.00×106 L storage tank at STP? Pt. B: How many grams of methane is this? Pt. C: How many grams of carbon dioxide gas could the same tank hold?

Answer #1

Part A

According to avogadro's law 1 mole of gas at STP occupy volume =
22.414 L then in 1.00 X 10^{6} L volume contain mole = 1.00
X 10^{6} / 22.414 = 44615 mole

**Tank contain 44615 mole of methane gas**

Part B

molar mass of methane = 16.04 gm/mole then 44615 mole of methane = 44615 X 16.04 = 715625 gm of methane

**tank contain 715625 gm of methane**

Part C

According to avogadro's law 1 mole of gas at STP occupy volume =
22.414 L then in 1.00 X 10^{6} L volume contain mole = 1.00
X 10^{6} / 22.414 = 44615 mole

44615 mole of CO_{2} in tank

molar mass of CO_{2} = 44.01 gm/mole then 44615 mole of
CO_{2} = 44615 X 44.01 = 1963506 gm of CO_{2}

**tank contain 1963506 gm of Carbon dioxide**

A 5.00 g mixture of methane (CH4) and ethane (C2H6) is combusted
in oxygen gas to produce carbon dioxide and water. If 14.09 g of
CO2 is produced, how many grams of methane was in the original 5.00
g mixture ?

A 18.0-L tank of carbon dioxide gas (CO2) is at a pressure of
9.60 ✕ 105 Pa and temperature of 21.0°C. (a) Calculate the
temperature of the gas in Kelvin. K (b) Use the ideal gas law to
calculate the number of moles of gas in the tank. mol (c) Use the
periodic table to compute the molecular weight of carbon dioxide,
expressing it in grams per mole. g/mol (d) Obtain the number of
grams of carbon dioxide in the...

A 22.0-L tank of carbon dioxide gas (CO2) is at a
pressure of 9.90 ? 105 Pa and temperature of 18.0°C.
(a) Calculate the temperature of the gas in Kelvin.
_______ K
(b) Use the ideal gas law to calculate the number of moles of gas
in the tank.
mol
(c) Use the periodic table to compute the molecular weight of
carbon dioxide, expressing it in grams per mole.
______ g/mol
(d) Obtain the number of grams of carbon dioxide...

Consider the following chemical reaction: CH4 + 2O2 → CO2 + 2H2O
4 moles of methane (CH4) are combined with 5 moles of oxygen (O2).
How much carbon dioxide (CO2) will form?

part a: How many moles of gas does a 1.00 L container is filled
with 1.52 atm N2, 0.12 atm O2, and 0.040 atm
CO2 gases at 25 °C?
part b: How many moles of N2 gas are there in a 1.0 L
container which contains 1.52 atm of N2 gas at 25
ºC?
part c: How many moles of O2 gas are there in a 1.0 L
container which contains 0.12 atm of O2 gas at 25
ºC?
part...

15.0 moles of gas are in a 4.00 L tank at 21.2 ∘C . Calculate
the difference in pressure between methane and an ideal gas under
these conditions. The van der Waals constants for methane are
a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.

12.0 moles of gas are in a 4.00 L tank at 24.4 ∘C . Calculate
the difference in pressure between methane and an ideal gas under
these conditions. The van der Waals constants for methane are
a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.

12.0 moles of gas are in a 4.00 L tank at 21.6 ∘C . Calculate
the difference in pressure between methane and an ideal
gas under these conditions. The van der Waals constants for methane
are a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.

15.0 moles of gas are in a 4.00 L tank at 20.1 ∘C . Calculate
the difference in pressure between methane and an ideal gas under
these conditions. The van der Waals constants for methane are
a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.

14.0 moles of gas are in a 8.00 L tank at 21.0 ∘C . Calculate
the difference in pressure between methane and an ideal
gas under these conditions. The van der Waals constants for methane
are a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.

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