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How would the equilibrium change in the temperature were increased in so2g?
Increasing the temperature of the system involving sulfur dioxide (SO2) in equilibrium would shift the equilibrium position according to Le Chatelier's principle. If the reaction is endothermic (absorbs heat), the equilibrium will shift to the right, favoring the formation of products. Conversely, if the reaction is exothermic (releases heat), the equilibrium will shift to the left, favoring the reactants. Therefore, the specific direction of the shift depends on the nature of the reaction involving SO2.
For the reaction 2 hclaq plus k2so3s h2ol plus so2g plus 2 kclaq answer the following questions how many grams of k2so3s would be required to react completely with 150.0 ml of 0.353 m hcl?
If you added less than the amount needed in part (b) of K2SO3, what would be the limiting reactant? If you added more than the amount needed in part (b) of K2SO3, what would be the limiting reactant? Which situation would create the most SO2 gas?excess HClexcess K2SO3 excess H2Oexcess KClperfectly matched amounts of HCl and K2SO3
