1- Write out the chemical reaction that occurs when an aqueous solution of iron(

Question

1- Write out the chemical reaction that occurs when an aqueous solution of iron(III)nitrate reacts with an aqueous solution of potassium iodide to produce an aqueous solution of iron(III)iodide and an aqueous solution of potassium nitrate.

2- Is the reaction in question 1 an example of a precipitation reaction? Explain.

3- Predict the products for the reaction that occurs when an aqueous solution of lead(II)nitrate (Pb(NO3)2) reacts chemically with an aqueous solution of potassium iodide (Kl).

4- Write balanced chemical reactions for each of the following:

Al (s) + HNO3 (aq) ----> Al(NO3)3 (aq) + H2 (g)

Sodium sulfate + barium nitrate ----> barium sulfate + sodium nitrate

Calcium carbonate + heat ----> calcium oxide + carbon dioxide

Potassium + chlorine ----> potassium chloride

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Explanation / Answer

3 Pb(NO3)2(aq)+2NaI(aq)=2NaNO3(aq)+PbI2(s)

2Al (s) + 6HNO3 (aq) ? 2Al(NO3)3 (aq) + 3H2 (g)

Na2So4+ barium nitrate ? barium sulfate + sodium nitrate   BaNO3 + Na2SO4 -> BaSO4 + 2 NaNO3, or simply   Ba(2+) + SO4(2-) -> BaSO4

a) CaCO3 -----> CaO + CO2

b) The molar mass of CaCO3 is 100.1 g/mol.
12.25 g CaCO3 x (1 mol / 100.1 g ) = 0.1224 mol CaCO3
1 mol CaCO3 produces 1 mol CaO
0.1224 mol CaCO3 x (1 mol CaO / 1 mol CaCO3) = 0.1224 mol CaO
The molar mass of CaO is 56.1 g/mol.
0.1224 mol CaO x (56.1 g / 1 mol) = 6.87 g CaO

c) 1 mol CaCO3 produces 1 mol CO2 gas.
0.1224 mol CaCO3 x (1 mol CO2 / 1 mol CaCO3 ) = 0.1224 mol CO2
Use the ideal gas law to find the volume.
V = nRT/P = (0.1224 mol x 0.08206 L atm / K mol x 283 K) / 0.95 atm = 29.9 L

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