calculate the amount of heat required to decompose 8 mol of NaHCO3(s)
2NaHCO3(s) + 94000 J = Na2CO3(s)+ H2O(g) + CO2(g)
To calculate the amount of heat required to decompose 8 mol of NaHCO3 (s), you need to use the stoichiometry of the reaction equation provided.
From the balanced chemical equation:
2NaHCO3(s) + 94000 J = Na2CO3(s) + H2O(g) + CO2(g)
We can see that for every 2 moles of NaHCO3 decomposed, 94000 J of heat is released.
Therefore, the heat released per mole of NaHCO3 decomposed is:
94000 J / 2 mol = 47000 J/mol
Now we can calculate the amount of heat required to decompose 8 mol of NaHCO3:
Heat required = 47000 J/mol × 8 mol = 376000 J
To calculate the amount of heat required to decompose 8 mol of NaHCO3(s), we first need to determine the molar heat of the reaction. The equation you provided shows that the decomposition of 2 moles of NaHCO3(s) releases 94000 J of heat energy.
We can set up a proportion to find the heat of decomposition for 8 moles of NaHCO3(s):
2 mol : 94000 J = 8 mol : x J
Cross multiplying, we have:
2 * x = 8 * 94000
2x = 752000
x = 752000 / 2
x = 376000 J
Therefore, the amount of heat required to decompose 8 moles of NaHCO3(s) is 376,000 J.
Look up the delta H formation for the materials in your text/notes. Then
dH rxn = (n*dHo formation products) - (n*dHo formation reactants)