Final answer:
To find the number of moles of carbon disulfide (CS2) needed to react with 0.405 L of oxygen at STP, since 1 mole of any gas occupies 22.414 liters at STP, we calculate as follows: 0.405 L / 22.414 L/mol = 0.0181 moles of CS2.
Step-by-step explanation:
To determine the number of moles of carbon disulfide (CS2) needed to react with 0.405 L of oxygen at STP, we should first know the balanced chemical equation for the reaction between CS2 and O2. However, since this information is not provided in the question, we will use the fact that at STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22.414 liters. Therefore, we can find the moles of oxygen gas by dividing the volume of oxygen given by the molar volume at STP.
Using the formula:
Moles of oxygen = Volume of oxygen (L) / Molar volume at STP (22.414 L/mol)
We calculate:
Moles of oxygen = 0.405 L / 22.414 L/mol = 0.0181 moles
Assuming a simple reaction where one mole of CS2 requires one mole of oxygen (which is often not the case, but no reaction equation is given), the moles of CS2 needed would be equal to the moles of oxygen. Therefore, the answer would be 0.0181 moles of CS2.