Consider the chemical reaction: 2 H₂O(l) → 2 H₂(g) + O₂(g) What mass of H₂O is required to form 1.85 L of O₂ at a temperature of 315 K and a pressure of 0.981 atm?

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Use the ideal gas law to find the number of moles of O2. The ideal gas law is given by the equation: \( PV = nRT \), where \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin.

Rearrange the ideal gas law to solve for \( n \): \( n = \frac{PV}{RT} \). Substitute the given values for \( P \), \( V \), and \( T \) into the equation to calculate the moles of O2.

Use the stoichiometry of the balanced chemical equation to find the moles of H2O required. According to the equation, 2 moles of H2O produce 1 mole of O2. Therefore, multiply the moles of O2 by 2 to find the moles of H2O needed.

Convert the moles of H2O to grams. Use the molar mass of H2O (approximately 18.02 g/mol) to convert moles to grams by multiplying the moles of H2O by the molar mass.

Summarize the steps and ensure all units are consistent throughout the calculations to find the mass of H2O required.

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주요 개념

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Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It allows us to determine the relationships between the amounts of substances involved. In this case, the balanced equation shows that 2 moles of water produce 1 mole of oxygen, which is essential for calculating the required mass of water.

Ideal Gas Law

The Ideal Gas Law (PV = nRT) relates the pressure, volume, temperature, and number of moles of a gas. It is crucial for converting the volume of oxygen gas produced into moles, which can then be used in stoichiometric calculations. Understanding this law helps in determining how many moles of O2 correspond to the given conditions of temperature and pressure.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. It is necessary for converting between moles and grams in stoichiometric calculations. For water (H2O), the molar mass is approximately 18.02 g/mol, which will be used to find the mass of water needed to produce the desired amount of oxygen.

Consider the chemical reaction: 2 H2O(l) → 2 H2(g) + O2(g) What mass of H2O is required to form 1.85 L of O2 at a temperature of 315 K and a pressure of 0.981 atm?