Acetylene gas, c2h2, burns in oxygen to produce carbon dioxide and water. if 60.5 g co2 are produced when 22.6 g c2h2 react with sufficient oxygen, what is the percent yield for the reaction?

-

79.11%

Explanation: -

Actual mass of CO₂ = 60.5 g

Molar mass of CO₂ = 12 x 1 + 16 x 2 = 44 g / mol

Actual number of moles of CO₂ =

= 1.375 mol of CO₂

Mass of C₂H₂ = 22.6 g

Molar mass of C₂H₂ = 12 x 2 + 1 x 2

= 26 g / mol

Number of moles of C₂H₂ =

= 0.869 mol

The balanced chemical equation for the reaction is

2 C₂H₂ + 5 O₂ → 4 CO₂ + 2 H₂O

From the equation we see that

2 mol of C₂H₂ gives 4 mol of CO₂

0.869 mol of C₂H₂ gives

= 1.738 mol of CO₂

Percentage yield = x 100

=79.11%

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.