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1.002 g of dysprosium chromate decahydrate (formula weight 853.11g/mol) will dissolve in 100 ml of water at 25oC. When 2.00 grams of dysprosium chromate decahydrate is added to 100 ml of water the equilibrium below is established.
Dy2(CrO4)3 .10H2O (s) <===> 2Dy3+(aq) + 3CrO42-(aq). +10H2O (l)
What will be the equilibrium constant for this reaction?
How do the following changes affect the value of the equilibrium constant for a gas-phase exothermic reaction: 1. removal of a reactant
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aqueous solutions of ironiii chloride and sodium hydroxide are mixed together to form a combined solution that is 0.015
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if H2 of 50.0 mL and C 2 H 4 of 50.0 mL are permitted to react at the pressure of 1.5 atm, produce C 2 H 6 that has a volume of 50.0 mille litres.. compute the amount of (PV )work done?
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