The reaction is:
NH4 (NO3) (s) ⇄ N2O (g) + 2 H2O (g)
This means that 1 mol of NH4 (NO3)s produces 3 moles of gases.
Now find the number of moles in 1.71 kg of NH4 (NO3)
Molar mass = 2*14g/mol + 4 * 1g/mol + 3*16g/mol = 80 g/mol
# moles = mass / molar mass = 1710 g / 80 g/mol = 21.375 mol of NH4(NO3)
We already said that every mol of NH4(NO3) produces 3 moles of gases, then the number of moles of gases produced is 3 * 21.375 = 64.125 mol
Now use the equation for ideal gases to fin the volume
pV = nRT => V = nRT / p = (64.125 mol)(0.082atm*liter / K*mol) * (119 +273)K / (731mmHg *1 atm/760mmHg) =
V = 2143.01 liters
Answer:
For example, 0.9% NaCl contains 0.9 g NaCl per 100 ml of solution or 9 g NaCl/l. This can be converted to molarity by dividing by molecular weight: 0.9% NaCl = (9g/l)/(58.5g/mole) = 0.15 M NaCl.
Explanation:
Given parameters:
Mass of aspirin = 0.45g
Mass of C = 0.27g
Mass of H = 0.02g
Mass of O = 0.16g
Unknown:
Mass percentage of the constituents = ?
Solution:
To find the mass percent, ensure that sum of the mass of the elements add up to the that of the given mass of aspirin
Total mass = 0.27 + 0.02 + 0.16 = 0.45g
Now express each of the given percentages to that of the total one.
mass percent of C = 
x 100 = 60%
mass percent of H = 
x 100 = 4.4%
mass percent of O = 
x 100 = 36%
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