A full syringe contains this equilibrium: 2 NO₂(g) N₂O4(g) If nitrogen dioxide gas is brown and the other gas is colourless, what is observed when the syringe is used to compress this gas mixture? Select one: O a. The mixture gets darker. O b. The mixture gets darker, then lighter. O C. The mixture get lighter, then darker. O d. The mixture gets lighter.

A full syringe contains this equilibrium: 2 NO₂(g) N₂O4(g) If nitrogen dioxide gas is brown and the other gas is colourless, what is observed when the syringe is used to compress this gas mixture? Select one: O a. The mixture gets darker. O b. The mixture gets darker, then lighter. O C. The mixture get lighter, then darker. O d. The mixture gets lighter.

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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Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO₂ is a reddish brown gas while N₂O4 is colorless. At high temperature the red color is strong. At low temperature the gas has less color. If we represent the equilibrium as: 2 NO2 (9) N₂O4 (9) We can conclude that: 1. This reaction is O exothermic. O endothermic. O neutral. O More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: O increases. O decreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of N₂O4: O increases. O decreases. O remains the same. O More information is needed to answer this question.
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A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant. A(s) B(g) + C(g) Then, the container volume was doubled and equilibrium was re-established. How many moles of A remain? moles of A: mol
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Consider the following equilibrium: Caco3(s) = Ca0(s) + CO2(g) AH = 1170 kJ Which of the following will shift the equilibrium to the left? X. adding CaO(s) Y. removing CO2(g) Z. cooling the system O Xand Y only O Yonly Y and Z only X and Z only O Xonly
3H2(g) + N2(g) ⟷⟷ 2NH3(g) + Heat
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