Strontium metal is responsible for the red color in fireworks. Fireworks manufacturers use strontium carbonate, which can be produced by combining strontium metal, graphite (C), and oxygen gas. The formation of one mole of SrCO3 releases 1.220 x 10^3 kJ of energy.
a) Write the balanced thermochemical equation for the reaction.
b) What is delta-H when 10.00 L oxygen at 25 degrees C and 1 atm is used in the reaction?
Does my work make sense?
a) 2/3Sr + 2/3C + O2 --> 2/3SrCO3
b) ideal gas constant = .08206 L atm/mol K
10.00 L * 1.00 atm/ x mol * 298.2 = .08206
.03353x mol O2= .08206
mol O2= 2.447
3(2.447)= 2x
7.341 = 2x
x= 3.67 mol
delta-H = 1.220 x 10^2 kJ * 3.67 mol= 4.48 x 10^3 kJ
If this is wrong, how do I approach the problem?
moles O2=PV/RT
= 1*10/.082*298 which is not your answer.
so if that amount of O2 is used, you get
you get molesO2/1 * 2/3*1.22E3kJ of energy.
1 answer
sucker, u have to cross multiply the values
1 answer