What mass of carbon dioxide is produced from the complete combustion of 8.10 10 <UNK> 3 g methane?
Thus, the mass of carbon dioxide produced from the complete combustion of 8.10×10−3 g of methane is 2.22×10–2 g.
How do you calculate the mass of carbon dioxide produced?
To find the mass of carbon dioxide used, we can use the number of moles from the above equation, and the molecular weight of CO2 (= 44.009 g/mol). The mass of CO2 produced is 3.29*10^-3g.
What mass of CO2 is produced by the complete combustion of 52 grams of c2 h2?
Is this balanced? Don’t trust my ‘rithmetic! Given the stoichiometry, we gets 4⋅mol CO2(g) given complete combustion, a mass of 4⋅mol×44.0⋅g⋅mol−1=176⋅g carbon dioxide………. Take that atmosphere!
What did you calculate for mass of CO2 produced?
For oxygen, we get 15.999 AMUs, reflecting the fact the almost all oxygen atoms have 8 protons and 8 neutrons. Therefore, CO2 has an atomic mass of 12.011 + 2(15.999) = 44.009 AMUs. In more convenient units, one mole of CO2 would weigh 44.009 grams.
What mass of carbon dioxide is produced from the complete combustion of methane?
As we can see here, the mole ratio between methane (CH4) and carbon dioxide (CO2) is 1:1 , i.e. one mole of methane will produce one mole of carbon dioxide in return. In here, we burn 2.6⋅10−3 g of methane.
What will be the mass of one molecule of CO2?
1 mole of any substance contains 6.022 × 10^23 (Avogadro number) fundamental units. 1 mole CO2 contains 6.022×10^23 molecules of CO2. So, mass of 6.022 × 10^23 molecules = 44 g. Mass of one molecule of CO2 = 44/(6.022×10^23) g = 7.3 × 10^-23 g.
What volume of oxygen is required for the complete combustion?
1 Mole of acetylene requires 2.5 moles of oxygen for complete combustion. At NTP , 22.4 Litres of acetylene requires= 2.5 x 22.4 Litres of oxygen. So 200 ml of acetylene at NTP requires= 0.2/22.4 x 2.5 x 22.4 Litres of O2 = 0.5 Litres= 500 ml.