Answer:
This is a simple stoichiometry problem using the ideal gas law.
First, take the grams of ammonium carbonate and convert it to moles using its molar mass and dividing. 11.9 g/96.0932 g/mol= .12384 mol
Now use a molar conversion using the balanced equation,
1 mol (NH4)2CO3 ---> 4 mol gas formed (2 mol NH3 + 1 mol CO2 + 1 mol H2O) = .12384 x 4 = .49535 mol gas
PV=nRT
V=nRT/P= .49535mol (.08206 Lxatm/molxK) (296K)/ (1.03 atm)=11.682 L
Explanation:
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Can I get Braineist.
Stoichiometry is used to determine the mass and the moles of the reactants and the products. 48 gms of ammonium carbonate is required to produce 1 mole of ammonia.
Stoichiometry coefficients are the numbers before the molecules of the reactant or the product side of the reaction that presents the numerical quantity of the chemical species.
The balanced chemical reaction is given as:
(NH₄)2CO₃ → 2 NH₃ + CO₂ + H₂0
Hence, 2 moles of ammonia are produced from 1 mole of ammonium carbonate. So, 0.5 moles of ammonium carbonate will be needed to produce 1 mole of ammonia.
Mass of ammonium carbonate is calculated as:
Mass = moles × molar mass
= 0.5 mol × 96.09 g/mol
= 48 gm
Therefore, 48 gm of ammonium carbonate is required to produce 1 mole of ammonia.
Learn more about moles and mass here:
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