1. The combustion of acetylene gas is represented by the equation: 2C2H2(g)+ 5 O2(g) 4CO2(g) + 2H2O (g) . How many grams of carbon dioxide (CO2) and grams of water(H2O)are produced when 66.0 g of C2H2 burns in oxygen? 2. If there are 35.o grams of C6H10 and 45.0 grams of O2, how many grams of the excess reagent will remain after the reaction ceases? 6 C6H10 +17 O2 12 CO2 + 10 H2O 3. For the balanced equation below, if the reaction of 77.0 grams of CaCN2 produces 27.1 g of NH3, what is the percent yield? CaCN2 + 3 H2O CaCO3 + 2 NH3. I need an explanation to your answers everyone. Thank you so much.
1. M(C2H2) = 26 g/mol
m(C2H2) "= \\frac{66.0}{26}=2.538 \\;mol"
n(CO2) = 2n(C2H2) "= 2 \\times 2.538 = 5.076 \\;mol"
M(CO2) = 44 g/mol
m(CO2) "= 44 \\times 5.076 = 223.34 \\;g"
n(H2O) = n(C2H2) = 2.538 mol
M(H2O) = 18 g/mol
m(H2O) "= 18 \\times 2.538 = 45.68 \\;g"
2. M(C6H10) = 82 g/mol
n(C6H10) "= \\frac{35.0}{82}=0.426 \\;mol"
M(O2) = 32 g/mol
n(O2) "= \\frac{45.0}{32}=1.406 \\;mol"
Theoretical proportion:
C6H10 : O2 = 6 : 17 = 1 : 2.83
Real proportion:
C6H10 : O2 = 0.426 : 1.406 = 1 : 3.3
So, C6H10 is the limiting reactant.
According to the reaction:
n(O2) "= \\frac{17}{6}n(C_6H_{10}) = \\frac{17}{6} \\times 0.426 = 1.207 \\;mol"
Used mass of O2:
m’(O2) "= 1.207 \\times 32 = 38.624 \\;g"
Δm(O2) = 45.0 – 38.624 = 6.376 g
So, 6.376 g of O2 (excess reagent) will remain after the reaction ceases.
3. M(CaCN2) = 80 g/mol
n(CaCN2) "= \\frac{77.0}{80}= 0.9625 \\;mol"
According to the reaction:
n(NH3) = 2n(CaCN2) "= 2 \\times 0.9625 = 1.925 \\;mol"
M(NH3) = 17 g/mol
m’(NH3) = "1.925 \\times 17" = 32.725 g (theoretical mass)
Proportion:
32.725 – 100 %
27.1 – x
"x =\\frac{27.1 \\times 100}{32.725} = 82.81\\; \\%"
So, he percent yield is 82.81 %.
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