Question 5 Copper(II) nitrate crystallises as a hydrate Cu(NO3)2 ' x H20 In order to determine the number of mole of water in a mole of the hydrate, 2.416 g of the blue, hydrated crystals was carefully heated to remove the water, 1.876 g of the anhydrous Cu(NO3)2 was left. (a) Write a balanced equation for the heating of Cu(NO3)2 X H2O. (b) Use these data to determine the value of x (the number of mole of water per mole of Cu(NO3)2 x H2O. (x = 3) %3D (c) Unfortunately, one student heated the compound too strongly and some of the copper(II) nitrate decomposed to produce NO2(E) and O2(e) Balance the equation for the decomposition: Cu(NO3)2(5) CuO(s) NO2(8) O2(e)

Elemental iron is produced according to the following reaction: Fe2O3(s)  + Al(s) ---> Al2O3(s) + Fe(s) If 5.34 g Fe2O3 is allowed to react with excess Al, what is the theoretical yield of elemental iron for this reaction?    A) 0.934 g B) 1.87 g C) 3.73 g D) 6.82 g

Which of the metals (Fe, Zn, Mg) will react in an aqueous solution of AL(NO3)3 to produce aluminum meatal?

A3) Balance the following equation. You must enter a number in every blank. Fe(s) + O2lg) → Fe3O4(s)

What is the balanced equation for C4H10 (I) + O2(g) ---->