teeheequeen
New member
1. when ammonium nitrate is heated, it decomposes to give nitrogen gas. this property is used to inflate some balls.
a. write a balanced equation for this reaction (i think i got this part - NH4NO2 --> N2 + 2H2O)
b. calculate the grams of ammonium nitrate need to inflate a tennis ball to a volume of 86.2 mL at 1.20 atm and 22.0 degrees C (here, would i use PV = nRT and plug in the given numbers to determine moles and then work my way back to the ammonium nitrate then convert to grams?)
Also, I DID this problem, but I'm concerned about the answer I got:
2. calculate the real and ideal pressure of hydrogen gas at 891 degrees C if you have 2.00 mol of this gas at a volume of 5.00 L. find the percent error.
with number 2, my ideal is 38.2 and my real is 38.3. when i find the difference and divide by real to determine percent error, i get 0.002617..., but with significant figures considered, that's just a 0, isn't it? or would i say 2.61 * 10^ -3 or just round up to 1%
a. write a balanced equation for this reaction (i think i got this part - NH4NO2 --> N2 + 2H2O)
b. calculate the grams of ammonium nitrate need to inflate a tennis ball to a volume of 86.2 mL at 1.20 atm and 22.0 degrees C (here, would i use PV = nRT and plug in the given numbers to determine moles and then work my way back to the ammonium nitrate then convert to grams?)
Also, I DID this problem, but I'm concerned about the answer I got:
2. calculate the real and ideal pressure of hydrogen gas at 891 degrees C if you have 2.00 mol of this gas at a volume of 5.00 L. find the percent error.
with number 2, my ideal is 38.2 and my real is 38.3. when i find the difference and divide by real to determine percent error, i get 0.002617..., but with significant figures considered, that's just a 0, isn't it? or would i say 2.61 * 10^ -3 or just round up to 1%