A 0.693 g0.693 g sample of a metal, M, reacts completely with sulfuric acid according to   M(s)+H2SO4(aq)⟶MSO4(aq)+H2(g)M(s)+H2SO4(aq)⟶MSO4(aq)+H2(g)   A volume of 269 mL269 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal.

Carbon dioxide gas, CO2(g), is generated in the combustion of a sample of ethane (C2H6). This CO2 is all bubbled into aqueous barium hydroxide to be absorbed to produce 0.506 g of solid barium carbonate precipitate. How many grams of ethane (C2H6) were initially burned? The absorption-precipitation reaction is given by [CO2(g) + Ba(OH)2(aq)  BaCO3(s) + H2O(l)].

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation   MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g)   How much MnO2⁢(s) should be added to excess HCl(aq) to obtain 335 mL Cl2⁢(g) at 25 °C and 1.00×102 kPa ? mass: ______g MnO2

In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following balanced chemical equation: Pcl5(s)+4H2O(l) ---> H3PO4 (aq) + 5HCl (g) The molar masses for each compound in the equation are as follows;  PCl5: 208.224 g/mol H2O: 18.015 g/mol H3PO4: 97.994 g/mol HCl; 36.45 g/mol   Based on the information above and the information attached explain in WORDS why PCl5 is the limiting reagent.