Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N₂O4(9) ? 2 NO₂(g) Three experiments were run starting with different initial amounts of N₂O4(g) ([N₂O4lo in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter). For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO₂ and N₂04 at equilibrium. Be sure to round to the correct number of significant figures. Exp [N₂04]0 [NO₂] [N₂04] 1 3.8 2 3.1 3 2.1 2.98 2.3 2.64 1.8 2.06 1.1 [NO₂] 2 [NO₂] [N₂04] / [N₂04] [NO₂]² [N₂04] Based on your calculations, indicate whether each statement is True (T) or False (F): 1. Each experiment started with a different initial concentration of N₂O4. 2. The ratio ([NO₂] / [N₂O4]) is equal to a constant value. 3. The ratio (2 [NO₂] / [N₂O4]) is equal to a constant value. 4. The ratio ([NO₂]2/[N₂O4]) is equal to a constant value. 5. Each experiment reached a different set of equilibrium concentrations.

Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N₂O4(9) ? 2 NO₂(g) Three experiments were run starting with different initial amounts of N₂O4(g) ([N₂O4lo in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter). For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO₂ and N₂04 at equilibrium. Be sure to round to the correct number of significant figures. Exp [N₂04]0 [NO₂] [N₂04] 1 3.8 2 3.1 3 2.1 2.98 2.3 2.64 1.8 2.06 1.1 [NO₂] 2 [NO₂] [N₂04] / [N₂04] [NO₂]² [N₂04] Based on your calculations, indicate whether each statement is True (T) or False (F): 1. Each experiment started with a different initial concentration of N₂O4. 2. The ratio ([NO₂] / [N₂O4]) is equal to a constant value. 3. The ratio (2 [NO₂] / [N₂O4]) is equal to a constant value. 4. The ratio ([NO₂]2/[N₂O4]) is equal to a constant value. 5. Each experiment reached a different set of equilibrium concentrations.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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