Give the oxidation state of each metal species.   Fe−→−−−−−heatexcess COFe(CO)5−→−I2heatFe(CO)4I2

what type reaction is 2Fe+3H2SO4=Fe2(SO4)3+2H2

14.4 g of magnesium nitrate is dissolved in 1.20 L of water. 25 mL of this solution is taken and diluted to 175 mL with water. What is the final concentration of the nitrate ion?

Describe in words how you do the following preparation. Then give molecular equation for the preparation. MgCl2(s) from Mg(OH)2(s)

1. If you use 6.95 g of the CuSO 5 H₂O starting material, what mass in grams of the [Cu(NH3)4]SO4 H₂O product would you expect to isolate at the end of the reaction? Include 3 significant figures in your answer. This mass represents the theoretical yield of the product.

Write the balanced NET ionic equation for the reaction when (NH4)2CO3 and CaCl2 are mixed in aqueous solution. If no reaction occurs, simply write only NR.

7 The oxidation state of chlorine in ClO4- is A) 0 B) +5 C) -5 D) +7

10. Write the completed and balanced equation with the correct physical state for each species in molecular, ionic and net ionic form. CS3PO4 (aq) + Ge(C2H3O2)4 (aq) → lonic: Net lonic:

A yellow solid is either lead(II) chromate or sodium chromate. What would you do to tell which compound the solid is?

Consider the series of reactions to synthesize the alum (KAl(SO4 )2 · xH2O(s)) Assuming an excess of the other reagents, from one mole of aluminum Al (s), how many moles of alum will be produced?