The following set of reactions can be used to produce nitric acid, HNO3. Calculate the mass of nitric acid produced from the reaction of 15.5 kg of nitrogen gas with excess hydrogen gas. Each reaction in turn has an excess of the second reactant added.

N2(g) + 3 H2(g) ? 2 NH3(g)
4 NH3(g) + 5 O2(g) ? 4 NO(g) + 6 H2O(g) 2 NO(g) + O2(g) ? 2 NO2(g)
3 NO2(g) + H2O(l) ? 2 HNO3(aq) + NO(g)

For the following reactions:

Predict the products (if any). (If there is no reaction, state "no reaction" and do not write any equations.)

Write the balanced chemical equation including all phases.

Write the balanced complete ionic equation including all phases.

Write the balanced net ionic equation including all phases.

Circle the spectator ion(s) (if any).

Write the type of reaction (precipitation, acid?base forming a weak electrolyte or acid?base forming a gas).

(a) aqueouslithiumcarbonateandsulfuricacid?

(b) Mn(NO3)2(aq)+Na2CO3(aq)?

(c) Ti(ClO4)2(aq) + Na3PO4(aq)?

(d) NaOH(aq) + NH4Cl(aq)?

(e) Srl2(aq)+Na2SO4(aq)?

(f) aqueous lithium hydrogen sulfite and perchloric acid ?

(g) HNO3(aq) + Ca(OH)2(s)?

(h) Sn(C2H3O2)2(aq)+Cu(NO3)2(aq)?