Consider the following exothermic reversible reaction at equilibrium:SO3 (g) + NO (g) → SO₂ (g) + NO₂ (g)[balanced]Which of the following stresses will cause an increase in the number of moles of SO3?O Decrease the concentration of NO2 (g)O Increase the pressure by decreasing the volumeAdd a catalystO Increase the concentration of NOO Increase the temperature

Le chatelier principle states that equilibrium will shift in such a way so as to undo the effect of…

Consider the following exothermic reversible reaction at equilibrium: SO3 (g) + NO (g) SO2 (g) + NO2 (g) [balanced] Which of the following stresses will cause an increase in the number of moles of SO3? Decrease the concentration of NO2 (g) Increase the pressure by decreasing the volume O Add a catalyst O Increase the concentration of NO Increase the temperature

Consider the following exothermic reversible reaction at equilibrium: SO3 (g) + NO (g) SO2 (g) + NO2 (g) [balanced] Which of the following stresses will cause an increase in the number of moles of SO3? Decrease the concentration of NO2 (g) Increase the pressure by decreasing the volume O Add a catalyst O Increase the concentration of NO Increase the temperature

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 126CP: . Consider the following exothermic reaction at equilibrium: N2(g)+3H2(g)2NH3(g)Predict how the...

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. Consider the following exothermic reaction at equilibrium: N2(g)+3H2(g)2NH3(g)Predict how the following changes affect the number of moles of each component of the system after equilibrium is re-established by completing the table. Complete the table with the terms increase, decrease, or no change. N2 H2 NH3 Add N2(g) Remove H2(g) Add NH3(g) Add Ne(g) (constant V) Increase the temperature Decrease the volume (constant T) Add a catalyst
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