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...

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