The mass of carbon dioxide that is produced will be 31,671 grams or 31.671 kg
First, the equation of the reaction:
[tex]C_3H_8(g)+5O_2(g)-- > 3CO_2(g)+4H_2O(g)[/tex]
The mole ratio of propane burned to carbon dioxide produced is 1:3.
The density of propane gas is 0.621 g/mL, thus, 17.0 L of propane will weigh:
Density = mass/volume, mass = 0.621 g/mL x 17000 = 10,557 g
Mole of 10,557 g of propane = 10557/44.1 = 239.39 moles
Equivalent mole of carbon dioxide produced = 239.39 x 3 = 718.16 moles
Mass of 718.16 moles carbon dioxide = 718.16 x 44.1 = 31,671 grams or 31.671 kg
More on stoichiometric calculations can be found here: https://brainly.com/question/13384700
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