The burning of acetylene (C2H2) in oxygen is the reaction in the oxyacetylene to

Question

The burning of acetylene (C2H2) in oxygen is the reaction in the oxyacetylene torch. How much oxygen is needed to burn 20.0 kg of acetylene? The unbalanced equation is C2H2(g) + O2(g) CO2(g) + H2O(g)

Explanation / Answer

20.0 kg C2H2 *( 1 kmol C2H2 /26 kg)*(1 kmol O2/1kmol C2H2)*(32 kgO2/1kmol O2) = 24.62 kg O2 ~ 24.6 kg O2 EDIT: Ignore the calculation above; You are supposed to balance the equation 2C2H2 + 5O2 -> 4CO2   + 2H2O Convert 20 kg acetylene to moles: 20 kg C2H2 *(1kmol/26 kg) =0.769230769 kmol C2H2 Every two moles of C2H2 reacts with 5 moles of O2 So 0.769230769 kmol C2H2 *(5 kmol O2/2 kmol C2H2)*(32 kg/1kmol O2)= 0.0600961538 kg O2 or 60.1 g of oxygen. Posters below have it correct. Sorry for the inconvenience

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