A sample of nitrogen gas (N2) kept in a container of volume 13.3 L and at a temperature of 22.3°C exerts a pressure of 1.1 atm. Calculate the number of grams of gas present.

Question

A sample of nitrogen gas (N2) kept in a container of volume 13.3 L and at a temperature of 22.3°C exerts a pressure of 1.1 atm. Calculate the number of grams of gas present.

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2 answers
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Answer 1

DrBob222 answered
14 years ago

Use PV = nRT and solve for n = moles.

Then moles = grams/molar mass. You know moles and molar mass, solve for grams.

Answer 2

Explain Bot answered
11 months ago

To determine the number of grams of gas present, we need to use the ideal gas law equation, which relates the pressure (P), volume (V), temperature (T), and number of moles (n) of a gas:

PV = nRT

Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)

First, we need to convert the given temperature from Celsius to Kelvin. The Kelvin temperature scale is obtained by adding 273.15 to the Celsius temperature. Thus, 22.3°C + 273.15 = 295.45 K.

Now, we rearrange the ideal gas law equation to solve for the number of moles (n):

n = PV / RT

Substituting the given values:

n = (1.1 atm)(13.3 L) / (0.0821 L·atm/mol·K)(295.45 K)

Simplifying:

n = 18.058 mol

Since the molar mass of nitrogen (N2) is 28.014 g/mol, we can calculate the number of grams of gas present:

Number of grams = number of moles × molar mass

Number of grams = 18.058 mol × 28.014 g/mol

Number of grams ≈ 505.7 g

Therefore, the sample of nitrogen gas present in the container weighs approximately 505.7 grams.