A scuba diver’s tank contains 0.29 kg of O2 compressed into a volume of 2.3 L. b. What volume would this oxygen occupy at 26°C and 0.95 atm?

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Convert the mass of O2 to moles using the molar mass of O2. The molar mass of O2 is approximately 32 g/mol. Remember to convert the mass from kilograms to grams before using the molar mass.

Use the ideal gas law equation, PV = nRT, to calculate the volume at the new conditions. Rearrange the equation to solve for V (volume).

Convert the temperature from degrees Celsius to Kelvin by adding 273.15 to the Celsius temperature.

Insert the values for n (moles from step 1), R (the ideal gas constant, which is approximately 0.0821 L·atm/mol·K), T (temperature in Kelvin from step 3), and P (the pressure in atm) into the rearranged ideal gas law equation.

Calculate the volume V, which will be the volume the oxygen would occupy at 26°C and 0.95 atm.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ideal Gas Law

The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of a gas. It is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. This law allows us to predict the behavior of gases under various conditions.

Molar Mass and Moles

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To find the number of moles of a gas, you can use the formula n = mass/molar mass. In this question, knowing the molar mass of O2 (approximately 32 g/mol) is essential for converting the mass of oxygen into moles, which is necessary for applying the Ideal Gas Law.

Gas Behavior Under Different Conditions

Gases behave differently under varying conditions of temperature and pressure. According to the Ideal Gas Law, if the temperature increases, the volume of a gas will also increase if the pressure remains constant. Conversely, if the pressure increases, the volume will decrease. Understanding these relationships is crucial for solving problems involving gas volumes at different temperatures and pressures.

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