Question #5f0a2

1 Answer
May 11, 2016

Answer:

#"Grams of acetylene"# #~=# #2*g#

Explanation:

You have done the hard yards when you have the stoichiometric equation, which I note you have done:

#CaC-=C(s) + 2H_2O(l) rarr HC-=CH + Ca(OH)_2#

This equation explicitly says that #64.1*g# of calcium carbide react with #36*g# of water to produce #26*g# acetylene and #74*g# calcium hydroxide.

Each of these numbers represents molar equivalents of the reactants and products.

You started with #(5.00*g)/(64.1*g*mol^-1)# #=# #0.0780*mol# of calcium carbide. If follows that I formed an equivalent quantity of acetylene, i.e. #0.0780*mol#, and of calcium hydroxide.

So #"mass of acetylene = molar quantity"xx"molar mass"# #=# #0.0780*molxx26.0*g*mol^-1=??*g#

This reaction was the basis of the carbide lamp.