A mixture of 14.0 g of N2 and 3.024 g of H2 in a 5.00 L container is heated to 400 °C. Use the data in Appendix B to calculate the molar concentrations of N2, H2, and NH3 at equilibrium. Assume that ∆H° and ∆S° are independent of temperature, and remember that the standard state of a gas is defined in terms of pressure.

검증된 단계별 안내

Step 1: Write the balanced chemical equation for the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g).

Step 2: Calculate the initial moles of N2 and H2 using their given masses and molar masses (N2: 28.02 g/mol, H2: 2.02 g/mol).

Step 3: Set up an ICE (Initial, Change, Equilibrium) table to determine the changes in moles of N2, H2, and NH3 as the reaction reaches equilibrium.

Step 4: Use the equilibrium constant expression for the reaction, Kc = [NH3]^2 / ([N2][H2]^3), and the given temperature to find the equilibrium concentrations.

Step 5: Solve the equilibrium constant expression for the equilibrium concentrations of N2, H2, and NH3, using the changes in moles from the ICE table and the volume of the container (5.00 L).

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

11m

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Molar Concentration

Molar concentration, or molarity, is defined as the number of moles of solute per liter of solution. It is a crucial concept in chemistry for quantifying the concentration of reactants and products in a reaction. In this question, calculating the molar concentrations of N2, H2, and NH3 at equilibrium requires determining the number of moles of each gas and dividing by the volume of the container.

Equilibrium Constant (K)

The equilibrium constant (K) is a value that expresses the ratio of the concentrations of products to reactants at equilibrium for a reversible reaction. It is influenced by temperature and can be calculated using the concentrations of the gases involved. Understanding how to derive K from the reaction and apply it to find the equilibrium concentrations of N2, H2, and NH3 is essential for solving the problem.

Thermodynamic Data (ΔH° and S°)

Thermodynamic data, including standard enthalpy change (ΔH°) and standard entropy (S°), provide essential information about the energy changes and disorder associated with chemical reactions. These values are used to calculate the Gibbs free energy change (ΔG°), which helps predict the spontaneity of the reaction and the position of equilibrium. In this question, the provided thermodynamic data for N2O4 and NO2 will be necessary for determining the equilibrium state of the reaction.