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.

sucker, u have to cross multiply the values

Your approach to part a) of the problem is correct. The balanced thermochemical equation for the reaction is:

2/3 Sr + 2/3 C + O2 -> 2/3 SrCO3

However, your calculations for part b) are incorrect. Let's go through the correct approach to solve part b):

First, we need to find the number of moles of oxygen (O2) used in the reaction. We can use the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

Given:
Pressure (P) = 1 atm
Volume (V) = 10.00 L
Temperature (T) = 25 degrees Celsius = 298.15 K (Remember to convert to Kelvin)

Using the ideal gas law equation:
n = PV / RT
n = (1 atm * 10.00 L) / (0.08206 L.atm/(mol.K) * 298.15 K)

Simplifying:
n ≈ 0.409 mol

Now, we can use the stoichiometry of the reaction to find the number of moles of SrCO3 produced. From the balanced equation, we can see that for every 2/3 moles of oxygen used, 2/3 moles of SrCO3 are produced.

So, moles of SrCO3 produced = (2/3) * (0.409 mol)

Finally, we can calculate delta-H using the given value for the energy released per mole of SrCO3 formed:

delta-H = (1.220 x 10^3 kJ/mol) * (moles of SrCO3 produced)

Substituting the calculated value for moles of SrCO3 produced:
delta-H ≈ (1.220 x 10^3 kJ/mol) * (2/3) * (0.409 mol)

Evaluating this expression will give you the correct value for delta-H.

So, to summarize:

a) The balanced thermochemical equation for the reaction is:
2/3 Sr + 2/3 C + O2 -> 2/3 SrCO3

b) Using the correct calculations, you can find delta-H using the given information.