Assume that you have 1.65 g of nitroglycerin in a 614.0 mL steel container at 20

Question

Assume that you have 1.65 g of nitroglycerin in a 614.0 mL steel container at 20.0 C and 1.00 atm pressure. An explosion occurs, raising the temperature of the container and its contents to 425 C. The balanced equation is 4C3H5N3O9=12CO2+10H2O+6N2+O2 a)How many moles of nitroglycerin were in the container originally? b)How many moles of gas (air) were in the container originally? c)How many moles of gas are in the container after the explosion? d)What is the pressure (in atmospheres) inside the container after the explosion according to the ideal gas law?

Explanation / Answer

a) n =1.65/227 = 7.268 x10 ^-3 moles b)n =PV/RT = 0.025524 c)n = 0.025524 - 7.268 x10 ^-3 + (12+10+6+1)/4 x 7.268 x10 ^-3 = 0.07095 moles d)P/nT = constant P new = 6.617 atm

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