---
title: "The synthesis of sulfur trioxide from sulfur dioxide and oxygen gas is represented by the equation below. \\[ 2\\text{ SO}_2\\text{(g)} + \\text{O}_2\\text{(g)} \\rightleftharpoons 2\\text{ SO}_3\\text{(g)} \\quad \\Delta H^\\circ = -198\\text{ kJ/mol}_{\\text{rxn}} \\] A mixture of \\(\\text{SO}_2\\text{(g)}\\), \\(\\text{O}_2\\text{(g)}\\), and \\(\\text{SO}_3\\text{(g)}\\) is at equilibrium inside a rigid, sealed \\(2.0\\text{ L}\\) container at \\(600\\text{ K}\\). The temperature of the container is then increased to \\(800\\text{ K}\\). Which of the following correctly predicts the direction of the net reaction and the effect on the value of the equilibrium constant, \\(K_p\\), as the system establishes a new equilibrium?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/120281/"
date_modified: "2026-08-23T04:04:15+00:00"
---

# The synthesis of sulfur trioxide from sulfur dioxide and oxygen gas is represented by the equation below. \[ 2\text{ SO}_2\text{(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{ SO}_3\text{(g)} \quad \Delta H^\circ = -198\text{ kJ/mol}_{\text{rxn}} \] A mixture of \(\text{SO}_2\text{(g)}\), \(\text{O}_2\text{(g)}\), and \(\text{SO}_3\text{(g)}\) is at equilibrium inside a rigid, sealed \(2.0\text{ L}\) container at \(600\text{ K}\). The temperature of the container is then increased to \(800\text{ K}\). Which of the following correctly predicts the direction of the net reaction and the effect on the value of the equilibrium constant, \(K_p\), as the system establishes a new equilibrium?

The synthesis of sulfur trioxide from sulfur dioxide and oxygen gas is represented by the equation below. \[ 2\text{ SO}_2\text{(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{ SO}_3\text{(g)} \quad \Delta H^\circ = -198\text{ kJ/mol}_{\text{rxn}} \] A mixture of \(\text{SO}_2\text{(g)}\), \(\text{O}_2\text{(g)}\), and \(\text{SO}_3\text{(g)}\) is at equilibrium inside a rigid, sealed \(2.0\text{ L}\) container at \(600\text{ K}\). The temperature of the container is then increased to \(800\text{ K}\). Which of the following correctly predicts the direction of the net reaction and the effect on the value of the equilibrium constant, \(K_p\), as the system establishes a new equilibrium?

- **A.** Direction of net reaction: Toward products ; Value of \(K_p\): Increases
- **B.** Direction of net reaction: Toward products ; Value of \(K_p\): Decreases
- **C.** Direction of net reaction: Toward reactants ; Value of \(K_p\): Remains unchanged
- **D.** Direction of net reaction: Toward reactants ; Value of \(K_p\): Decreases

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120281/*