One method of manufacturing chlorine gas in a laboratory is to react manganese (IV) oxide with hydrochloric acid. MnO₂ (s) + 4 HCl(aq) → MnCl₂(aq) + 2 H₂O(l) + Cl₂(g) Calculate the volume, in litres, of chlorine gas produced as SATP if 50 6.00 mol/L HCI is reacted with excess MnO2. Do not show your work in the space provided. Only record your final answer with the correct number of significant the proper units. Answer:

Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.) Note: you are writing the molecular, and not the net ionic equation. → CaC1,₂(aq) + H₂O(1) X Ś

Consider the formation of chlorine gas, from household bleach (sodium hypochlorite) and hydrochloric acid.   NaClO(aq) + 2 HCl(aq) → Cl2(g) + H2O(l) + NaCl(aq) If 13.5 ml of sodium hypochlorite (d = 1.11 g/ml) reacts with excess hydrochloric acid, what volume of chlorine gas will be collected over water at 20.0 oC?  The lab barometer reads atmospheric pressure to be 755 mm Hg and the water vapor pressure at 20.0oC is 17.5 mm Hg.   Question  options:   4.05 L   4.75 L   4.39 L   4.99 L

Mining companies use this reaction to obtain iron from iron ore: Fe₂O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g) The reaction of 167 g Fe₂O3 with 85.8 g CO produces 72.3 g Fe. Determine the limiting reactant, theoretical yield, and percent yield. What volume (in mL) of 0.200 M NaOH do we need to titrate 35.00 mL of 0.140 M HBr to the equivalence point?