Question

a gas mixture is made by combining the 6.8 g of each Ar, Ne, and an unknown diatomic gas. At STP, the mixture occupies a volume of 16.80 L. What is the molar mass of the unknown gas? Identify the unknown gas: H2, Cl2, N2, F2, or O2.

Answer #1

A gas mixture is made by combining 6.1 g each of Ar, Ne, and an
unknown diatomic gas. At STP, the mixture occupies a volume of
12.12 L What is the molar mass of the unknown gas?Identify the
unknown gas.

A gas mixture is made by combining 6.16.1 g each of Ar, Ne, and
an unknown diatomic gas. At STP, the mixture occupies a volume of
12.1212.12 L.
What is the molar mass of the unknown gas?
Identify the unknown gas.

A gas mixture is made by combining 6.6 g each of Ar, Ne, and an
unknown diatomic gas. At STP, the mixture occupies a volume of
15.65 L. What is the molar mass of the unknown gas?

A gas mixture is made by combining 5.1 g each of Ar, Ne, and an
unknown diatomic gas. At STP, the mixture occupies a volume of
11.53 L. What is the molar mass of the unknown gas?

A gas mixture is made by combining 8.8 g each of Ar, Ne, and an
unknown diatomic gas. At STP, the mixture occupies a volume of
19.89 L.

1- A gas mixture is made by combining 6.9 g each of Ar, Ne, and
an unknown diatomic gas. At STP, the mixture occupies a volume of
15.60 L.
2- 1.85 g of an unknown gas at 21 °C and 1.10 atm is stored in a
1.65-L flask.
-What is the density of the gas?
-What is the molar mass of the gas?
3- An open flask sitting in a lab fridge looks empty, but we
know that actually it...

1. What is the molar mass of a gas if 0.252 g of the gas
occupies a volume of 125 mL at a temperature of 123°C and a
pressure of 778 torr?
2. A mixture of 0.229 g of H2, 1.08 g of
N2, and 0.836 g of Ar is stored in a closed container at
STP. Find the volume (in L) of the container, assuming that the
gases exhibit ideal behavior.

If a gaseous mixture is made by combining 3.02 g of Ar and 2.81
g of Kr in an evacuated 2.50 L container at 25.0 °C, what are the
partial pressures of each gas and what is the total pressure
exerted by the gaseous mixture? (All three
answers must be in units of atm)
PAr
PKr
PTotal

A mixture of Ar and N2 gases has a density of 1.477 g/L at STP.
What is the mole fraction of each gas?

At STP, air can be considered to be a mixture of ideal gases:
21.0% O2, 78.0% N2, and 1.00% Ar by volume.
a. Calculate the partial pressure of each gas at STP.
b. Calculate the density of air in g L at STP.

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