How many moles of oxygen gas are required to combust a #4*mol# quantity of acetylene completely?

2 Answers
anor277
Mar 11, 2016

#H-C-=C-H(g) + 5/2O_2(g) rarr 2CO_2(g) + H_2O(g)#

Explanation:

The balanced chemical equation is given. Each mole of acetylene requires two and a half moles of oxygen gas. So if 4 mol acetylene are combusted, some 10 moles of dioxygen are necessary.

Jarni Renz
Mar 11, 2016

#10# # mol# # O_2#

Explanation:

  1. First thing to do is to balance the chemical equation; The balanced equation is:
    #2C_2H_2 + 5O_2 rarr 4CO_2 + 2H_2O#

  2. Then use the coefficients, which represents the number of mol of its compound/molecules in said reaction, to get the number of mol of #O_2# molecules;

  3. Multiply the mol of acetylene as provided in the problem (#4 mol C_2H_2#) with the convertion ratio of the moles of acetylene and oxygen molecules (#(5 mol O_2)/(2mol C_2H_2#)) based on the balanced equation;
  4. Make sure to cancel the mole of #C_2H_2# and get your desired mole of #O_2# molecules.
  5. The answer per computation is 10 mol of #O_2#moleules
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