3. Chemical Reactions

According to the reaction Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g), what mass of Al2S3 remains unreacted when 20.00 g of Al2S3 and 2.00 g of H2O are reacted? The molar masses are: Al2S3 = 150.17 g/mol, H2O = 18.02 g/mol.

According to the following reaction, what mass of PbCl2 can form from 235 mL of 0.110 M KCl solution? Assume that there is excess Pb(NO3)2.2 KCl(aq) + Pb(NO3)2(aq) ⟶ PbCl2(s) + 2 KNO3(aq)

According to the following reaction, what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution?2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)

Ammonia gas decomposes according to the equation: 2NH3(g) → N2(g) + 3H2(g). If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced (also measured at STP)?

What is the balanced chemical equation for the reaction between salicylic acid (C7H6O3) and acetic anhydride (C4H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2)?

In the reaction 2C8H18(g) + 25O2(g) → 16CO2(g) + 18H2O(g), if 0.300 mol of octane (C8H18) is allowed to react with 0.870 mol of oxygen (O2) and oxygen is the limiting reactant, resulting in the production of 0.626 mol of water (H2O), how much octane is left unreacted?

C7H6O3 + C4H6O3 → C9H8O4 + CH3CO2H. How many grams of salicylic acid (C7H6O3) are needed to produce 11.9 g of aspirin (C9H8O4)?

CH3OH can be synthesized by the reaction CO(g) + 2H2(g) → CH3OH(g). How many liters of CO gas are required to produce 44.8 liters of CH3OH gas at STP?

Calculate how many moles of N₂ are produced when 2.4 mol of N₂H₄ completely react according to the balanced equation: 3 N₂H₄ → 4 NH₃ + 2 N₂.

Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. The balanced chemical equation is: 4HCl(aq) + MnO2(s) → MnCl2(aq) + 2H2O(l) + Cl2(g). A sample of 33.7 g of MnO2 is added to a solution containing 48.3 g of HCl. What is the limiting reactant?

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 = 63.02 g/mol.3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

Consider the following balanced reaction. What mass (in g) of CO2 can be formed from 288 mg of O2? Assume that there is excess C3H7SH present.C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g)

Consider the following reaction: 2 Mg + O2 → 2 MgO. What mass (g) of MgO can be created from 4.3 g of O2 and excess Mg?

Consider the following reaction:2 PbS (s) + 3 O2 (g) → 2 PbO (s) + 2 SO2 (g)ΔHrxn = -827.4 kJWhat mass of PbS has reacted if 853 kJ of heat is produced?

Consider the industrial conversion of ammonia to nitrogen monoxide: 2 N2H4(g) + 1 N2O4(g) → 3 N2(g) + 4 H2O(g). If H2O is produced at the rate of 0.66 mol/s, what is the rate of production of N2?