Question

Nitroglycerin is a powerful explosive that forms four different gases when it decomposes (i.e. when it explodes) as shown in the equation below. Calculate the volume in mL of nitrogen gas that will be collected at 1.25 atm and 112°C by the decomposition of 12.8 g of nitroglycerin, C3H5(NO3)3. Use the correct SF and units. 4 C3H5(NO3)3 (1) -->6 N2(g) + O2 (g) + 12 CO2 (g) + 10 H20 (g)

Answer 1

Males of Nitroglycerin = given mass molar mass = 12:& 9- . 227.0865 g/mol = 0.056366_ moles: 4 C3H5(NO3), - 6N2 192_----+--- According to balanced chemical equation 4 mole nilroglycerin produce + 6 mole N2 So, 1 mole " produce 6 mole No.

& 0.056366 mole nitroglycerin produce → 6 x 0.056366 mole Na 0.08455 mole Nz (g) the volume Now, we have to calculate of 0.08455 moles Ne gas. use, N = nRT - P given, moles of N2 (n) = 0.08455 Temperature, I = 112°C _ =_(112 + 273.15) K. 385:15 K. Pressure, P = 1.25 atm. Universal gas constant, R = 0.0820578 L-atm Kimol.

now, - V = nRX T = 0.08455 mol x 0.0820578 L'atm_X.385-15 k. 1.25 atm Kino V = 2.1377 L V = 2.1377 X 1000 me V = 2137 7 me. Volume of N2 gas will be 2137 7 me.