When ammonium nitrite (NH4NO2) is heated, it decomposes to give nitrogen gas. This property is used to inflate some tennis balls.
A. Write a balanced equation for the reaction.
B. Calculate the quantity in grams of NH4NO2 needed to inflate a tennis ball to a volume of 86.2 mL at 1.20 atm and 22 degrees C.
2006-09-02 18:15:53 · 2 answers · asked by Lorenz 2 in Science & Mathematics ➔ Chemistry
A.
___NH4NO2 ---> N2+ 2H2O
B.
___PV= nRT
___(1.20*101330)(86.2*10^(-6)) = n_N2(8.314)(22+273.15)
___n_N2 = 0.004271 mol
From the equation above, you can say that each 1 mol of NH4NO2 yields 1 mol of N2. Thus, we need 0.004271 mol of ammonium nitrite to produce 0.004271 mol of nitrogen gas:
___n_NH4NO2 = 0.004271 mol
The molecular mass of ammonium nitrite is:
___M_NH4NO2 = 2*M_N+ 4*M_H+ 2*M_O
___= 2*14.01+ 4*1.008+ 2*16.00 =
___= 64.052 g/mol
The amount in grams of NH4NO2 needed is
___n_NH4NO2*M_NH4NO2 = 0.004271*64.052 =
___= 0.273 grams
2006-09-02 19:13:37 · answer #1 · answered by Illusional Self 6 · 0⤊ 0⤋
step # one
calculate the unknown (x) moles of N2 from pv = nRT
n = pv / RT
step # two
find molar ratio by balancing the equation
Step # 3
calculate # of moles of NH4NO2 needed to produce the x moles of N2
2006-09-02 19:02:26 · answer #2 · answered by Roy G. Biv 3 · 0⤊ 1⤋