Question- Part 1) A 0.852 g sample of a liquid is vaporized. The vapor is found to occupy 153 mL at 110oC and 760 torr pressure. Calculate the molar mass of this chemical.
A) When an oxyacetylene torch burns, oxygen and acetylene react
5 O2(g) + 2 C2H2(g) à 4 CO2(g) + 2 H2O(g)
B) How many liters of C2H2 at STP are needed to produce 80.0 mL of CO2 at 500oC and 1.10 atm?
Part 2) How many grams of O2 are required to react with 10.0 L of acetylene at 0.989 atm and 20oC?
Part 3) Given that one mole of any gas occupies 22.4 L at 0oC and one atmosphere pressure, what volume of CO2 gas could be produced at the indicated conditions if a solid cube of graphite with a volume of 1.000 m3 was burned in O2 to produce CO2? The density of graphite is 2.25 g/mL.
If possible just a brief explanation how you got the answer?