The gas acetylene burns according to the equation: 2 C2H2 + 5 O2 > 2H2 + 4 CO2 If you have a 10.0 L tank of acetylene at 25.0 C and 1.00 atm, how many moles of CO2 will be produced if you burn all the acetylene in the tank?

The answer to your question is 0.82 moles of CO₂  

Explanation:

Data

V = 10L

T = 25°C

P = 1 atm

moles = n = ?

R = 0.08205 atm L/mol°K

Process

1.- Convert °C to °K

T = 25 + 273 = 298°K

2.- Use the ideal gas law to find the moles of Acetylene

    PV = nRT

Solve for n

    n = PV / RT

Substitution

     n = (1)(10) / (0.08205)(298)

Simplification

    n = 10 / 24.45

Result

     n = 0.409  moles of Acetylene

3.- Use proportions to find the moles of CO₂

                  2 moles of C₂H₂ 4 moles of CO₂

                  0.409 moles        x

                  x = (0.409 x 4) / 2

                  x = 1.636 / 2

                  x = 0.82 moles of CO₂      

specific gravity is the density of a substance divided by the density of water. since (at standard temperature and pressure) water has a density of 1 gram/cm3, and since all of the units cancel, specific gravity is usually very close to the same value as density

so "c" is the answer

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