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natita [175]
3 years ago
13

What is the pressure, in atm, exerted by 41.6 g oxygen in a 22.0L container at 30.0C ?

Chemistry
1 answer:
Reika [66]3 years ago
3 0

Answer:

1.47 atm

Explanation:

Step 1: Calculate the moles corresponding to 41.6 g of oxygen

The molar mass of oxygen is 32.00 g/mol.

41.6 g × 1 mol/32.00 g = 1.30 mol

Step 2: Convert 30.0 °C to Kelvin

We will use the following expression.

K = °C + 273.15 = 30.0 + 273.15 = 303.2 K

Step 3: Calculate the pressure exerted by the oxygen

We will use the ideal gas equation.

P × V = n × R × T

P = n × R × T / V

P = 1.30 mol × (0.0821 atm.L/mol.L) × 303.2 K / 22.0 L = 1.47 atm

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If we look at the intersection between -57°C and 1 atm, we can see that CO₂ is in the gas phase.

<em>At 10°C and 2 atm carbon dioxide is in the gas phase. From these conditions, how could the gaseous CO₂ be converted into liquid CO₂?</em>

Since at 10°C and 2 atm carbon dioxide is below the triple point, the only way to convert it into liquid is by increasing the pressure (moving up in the vertical direction).

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