# Problem: Ammonium carbonate decomposes upon heating according to the following balanced equation: (NH4)2CO3(s) → 2 NH3(g) + CO2(g) + H2O(g). Calculate the total volume of gas produced at 23.0˚C and 1.03 atm by the complete decomposition of 11.9 g of ammonium carbonate.

###### FREE Expert Solution

Recall the Ideal Gas Law equation:

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

Step 1. mol reactant

molar mass of (NH4)2CO3 = 96.09 g/mol

0.124 mol (NH4)2CO3

Step 2. volume of each product

$\mathbf{PV}\mathbf{=}\mathbf{nRT}\phantom{\rule{0ex}{0ex}}\frac{\overline{)\mathbf{P}}\mathbf{V}}{\overline{)\mathbf{P}}}\mathbf{=}\frac{\mathbf{nRT}}{\mathbf{P}}\phantom{\rule{0ex}{0ex}}\overline{){\mathbf{V}}{\mathbf{=}}\frac{\mathbf{nRT}}{\mathbf{P}}}$

P = 1.03 atm
T = 23.0˚C + 273.15 = 269.15 K
R = 0.08206 (L·atm)/(mol·K)

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###### Problem Details

Ammonium carbonate decomposes upon heating according to the following balanced equation: (NH4)2CO3(s) → 2 NH3(g) + CO2(g) + H2O(g). Calculate the total volume of gas produced at 23.0˚C and 1.03 atm by the complete decomposition of 11.9 g of ammonium carbonate.