Question

Calculate the density of oxygen, O₂, under each of the following conditions:

a. STP
b. 1.00 atm and 10.0 °C

A) a. 0.00243 g/L, b. 0.0112 g/L
B) a. 0.00143 g/L, b. 0.0232 g/L
C) a. 0.00143 g/L, b. 0.0112 g/L
D) a. 0.00243 g/L, b. 0.0232 g/L

Answer 1

To calculate the density of oxygen at STP and at 1.00 atm and 10.0 °C, the ideal gas law would be applied using oxygen's molar mass and the conditions provided. However, without the exact volume of oxygen gas at STP, an answer cannot be given.

Step-by-step explanation:

The student is asking to calculate the density of oxygen (₂O₂) under different conditions, specifically at standard temperature and pressure (STP) and at 1.00 atm with a temperature of 10.0 °C. To solve this, we would typically use the ideal gas law equation (PV=nRT), where P is pressure, V is volume, n is the number of moles, R is the universal gas constant, and T is temperature. Using the molar mass of oxygen (32.00 g/mol) and the appropriate values for R and T, we would calculate the volume that one mole of oxygen occupies under each set of conditions and then use this to find the density. However, as I do not have access to the necessary data to calculate the density at the specified conditions (like the volume of oxygen gas at STP).