Ammonium nitrate is a common ingredient in chemical fertilizers. Use the reaction shown to calculate the mass of solid ammonium nitrate that must be used to obtain 0.239 L of dinitrogen oxide gas at STP. NH4NO3(s) - N2O(g) + 2 H2O(g)
How would you start this problem?

Question

Ammonium nitrate is a common ingredient in chemical fertilizers. Use the reaction shown to calculate the mass of solid ammonium nitrate that must be used to obtain 0.239 L of dinitrogen oxide gas at STP.      NH4NO3(s)  -> N2O(g) + 2 H2O(g)
How would you start this problem?

xishem · Answer

How would you start it? Start by converting 0.239L of dinitrogen oxide gas into moles of gas using the ideal gas equation, PV=nRT.

anonymous · Answer

Then do you convert the other numbers, and plug in the answers?

xishem · Answer

From that you would convert from moles of N2O to moles of ammonium nitrate using a molar conversion factor, then to mass of ammonium nitrate using its molar mass.

anonymous · Answer

ok, thanks

xishem · Answer

Let me know how it works out.

rogue · Answer

At STP, 1 mol of gas is 22.4 L of gas, by the way. Makes life easier; you don't have to use PV=nRT ;)