Answer:
7.63 L is the produced volume of ammonia.
Explanation:
The balanced reaction of decomposition is this:
(NH₄)₂CO₃ (s) → 2NH₃ (g) + CO₂ (g) + H₂O (g)
We convert the mass of carbonate to moles → 15 g . 1mol / 96g = 0.156 mol
Ratio is 1:2, so the 0.156 moles will produce the double of moles of ammonia. → 0.156 . 2 = 0.312 moles
We use now, the Ideal Gases Law to determine the volume
Pressure . Volume = moles . R . T
T → 25.5°C + 273 = 298.5K
1 atm . V = 0.312 mol . 0.082 L.atm/mol.K . 298.5K
V = (0.312 mol . 0.082 L.atm/mol.K . 298.5K) / 1 atm → 7.63 L
Answer:
The total volume of ammonia gas is 7.65 L
Explanation:
Step 1: Data given
Temperature = 25.5 °C
Pressure = 1.0 atm
Mass of ammonium carbonate = 15.0 grams
Molar mass ammonium carbonate = 96.09 g/mol
Step 2: The balanced equation
(NH4)2CO3 (s) → 2 NH3 (g) + CO2 (g) + H2O (g)
Step 3: Calculate moles of (NH4)2CO3
Moles (NH4)2CO3 = mass (NH4)2CO3 / molar mass (NH4)2CO3
Moles (NH4)2CO3 = 15.0 grams / 96.09 g/mol
Moles (NH4)2CO3 = 0.156 moles
Step 4: Calculate moles NH3
For 1 mol (NH4)2CO3 we'll have 2 moles NH3, 1 mol CO2 and 1 mol H2O
For 0.156 moles (NH4)2CO3 we'll have 2*0.156 = 0.312 moles NH3
Step 5: Calculate volume of NH3 gas
p*V = n*R*T
⇒ with p = the pressure = 1 atm
⇒ with V = the volume of NH3 gas = TO BE DETERMINED
⇒ with n = the moles of NH3 gas = 0.312 moles
⇒ with R = the gas constant = 0.08206 L*atm/ mol*K
⇒ with T = The temperature = 25.5 °C = 298.65 K
V = (n*R*T)/p
V = (0.312 * 0.08206 * 298.65) / 1
V = 7.65 L
The total volume of ammonia gas is 7.65 L
