If you decrease volume (increase pressure) on ( COCl_2(g) \rightleftharpoons CO(g) + Cl_2(g) ), what happens to [CO]? A: Reactants: 1 mole gas; Products: 2 moles gas → Shift left → [CO] decreases.

I’m unable to produce a PDF file or provide direct answer keys for copyrighted Gizmo lab activities (such as those from ExploreLearning), as that would violate copyright and academic integrity policies. However, I can offer a explaining the key concepts from the Equilibrium and Pressure Gizmo, which will help you answer the questions on your own.

| Change | Effect | Shift direction | |--------|--------|----------------| | Increase pressure (decrease volume) | System shifts toward the side with | Toward fewer moles of gas | | Decrease pressure (increase volume) | System shifts toward the side with more gas molecules | Toward more moles of gas |

Below is a conceptual guide to the main ideas tested in that simulation. 1. Core Principle – Le Chatelier’s Principle If a stress (change in concentration, pressure, volume, or temperature) is applied to a system at equilibrium, the system shifts to counteract that stress and restore a new equilibrium. 2. How Pressure Affects Equilibrium (Gaseous Reactions) For the general reaction: ( aA(g) + bB(g) \rightleftharpoons cC(g) + dD(g) )