Calculate the volume of carbon (IV)oxide measured at s.t.p, produced when 1 kg of potassium hydrogen trioxocarbonate (IV) is totally decomposed by heat?(G.M...
Calculate the volume of carbon (IV)oxide measured at s.t.p, produced when 1 kg of potassium hydrogen trioxocarbonate (IV) is totally decomposed by heat?(G.M.V. at s.t.p 22.4 dm3, K = 39, O = 16, C = 12, H = 1)
Answer Details
The question is asking for the volume of carbon dioxide produced when 1 kg of potassium hydrogen trioxocarbonate (IV) is decomposed at standard temperature and pressure (STP). We can start by writing the balanced chemical equation for the decomposition of potassium hydrogen trioxocarbonate (IV):
2KHCO3(s) → K2CO3(s) + H2O(g) + CO2(g)
From this equation, we see that for every 2 moles of potassium hydrogen trioxocarbonate (IV) decomposed, 1 mole of carbon dioxide is produced. The molar mass of KHCO3 is:
1(39) + 1(12) + 3(16) = 100 g/mol
Therefore, 1 kg (1000 g) of KHCO3 is equal to:
1000 g / 100 g/mol = 10 mol
Since 2 moles of KHCO3 produce 1 mole of CO2, the number of moles of CO2 produced is:
10 mol / 2 = 5 mol
At STP, 1 mole of any ideal gas occupies 22.4 dm^3. Therefore, the volume of CO2 produced is:
5 mol x 22.4 dm^3/mol = 112 dm^3
So the answer is 112 dm^3. Therefore, the correct option is:
- 112 dm^3