Ammonium nitrate decomposes explosively at high temperatures to form nitrogen, oxygen, and water vapor. 2NH4NO3-->2N2+4H2O+O2. Calculate the number of grams of water formed when 25 L of N2 is produced in this reaction (assume STP)

zinc hyrdoxide + phosphoric acid --> zinc phosphate + water

To calculate the number of grams of water formed when 25 L of N2 is produced in the reaction, we need to use the ideal gas law and stoichiometry.

1. Convert 25 L of N2 to moles:
Using the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature, we can rearrange the equation to solve for n:
n = PV / RT.
Since the reaction takes place at standard temperature and pressure (STP), which is 1 atm and 273 K respectively, and nitrogen (N2) is the main component, we can use those values for the calculation.

n = (1 atm * 25 L) / (0.0821 L*atm/mol*K * 273 K)
n = 0.993 mol

2. Determine the moles of water formed:
From the balanced equation, we can see that for every 2 moles of NH4NO3, 4 moles of H2O are produced. Therefore, the ratio of moles of water to moles of nitrogen is 4/2 or 2.

moles of water = 0.993 mol * (2 mol H2O / 2 mol N2)
moles of water = 0.993 mol

3. Calculate the mass of water formed:
The molar mass of water (H2O) is 18 g/mol. Therefore, we can calculate the mass of water using the following equation:

mass of water = moles of water * molar mass of water
mass of water = 0.993 mol * 18 g/mol
mass of water = 17.874 g

Therefore, approximately 17.874 grams of water are formed when 25 L of N2 is produced in the given reaction at STP.