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 25 C and 1.07atm by the complete decomposition of 11.86 g of ammonium carbonate.
1. You have the balanced equation.
2. Convert 11.86 g (NH4)2CO3 t moles. moles = grams/molar mass.
3. Using the coefficients in the balanced equation, convert moles (NH4)2CO3 to
a. moles NH3,
b. moles CO2,
c. moles H2O.
4. Use PV = nRT with total moles = n.
Check my thinking.
how do you convert the moles of nh3 co2 ang h2o? is it just 2 mol nh3 1 mol co2 and 1 mol h20?
moles (NH4)2CO3 = 11.86/78.048 = about 0.15
Convert moles (NH4)2CO3 to moles CO2.
0.15 mols (NH4)2CO3 x (1 mol CO2/1 mol (NH4)2CO3 = 0.15 x (1/1) = etc.
To calculate the total volume of gas produced by the complete decomposition of ammonium carbonate, we need to use 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 ideal gas constant, and T is the temperature in Kelvin.
Let's first determine the number of moles of each gas produced by the decomposition reaction:
From the balanced equation, we can see that for every 1 mole of (NH4)2CO3 decomposed, 2 moles of NH3, 1 mole of CO2, and 1 mole of H2O are produced.
1 mole of (NH4)2CO3 has a molecular weight of:
(N) x 2 + (H) x 8 + (C) + (O) x 3 = 14 x 2 + 1 x 8 + 12 + 16 x 3 = 96 g/mol.
Given that we have 11.86 g of ammonium carbonate, we can calculate the number of moles by dividing the mass by the molecular weight:
n(CO2) = n(H2O) = n((NH4)2CO3) / molecular weight((NH4)2CO3) = 11.86 g / 96 g/mol.
n(NH3) = 2 x n((NH4)2CO3) / molecular weight((NH4)2CO3) = 2 x (11.86 g / 96 g/mol).
Next, we need to convert the temperature from Celsius to Kelvin:
T = 25°C + 273.15 = 298.15 K.
We are given that the pressure is 1.07 atm.
Now we can substitute the known values into the ideal gas law equation to solve for the volume (V), with n being the sum of moles of NH3, CO2, and H2O:
PV = nRT.
V = (n(NH3) + n(CO2) + n(H2O)) x RT / P.
Substituting the values:
V = [(2 x (11.86 g / 96 g/mol) + 11.86 g / 96 g/mol + 11.86 g / 96 g/mol) x 0.08206 L atm mol^-1 K^-1 x 298.15 K] / 1.07 atm.
Simplifying the equation and solving for V, we can find the total volume of gas produced upon the complete decomposition of ammonium carbonate.
Remember to convert grams to moles before substituting into the equation and to convert the result from liters (L) to the required unit if needed.