a)
Convert 15.9 L C2H2 to moles. moles = L/22.41.
Convert moles C2H2 to moles CO2 using the coefficients in the balanced equation.
b)
Convert 59.3 mL O2 to moles, convert moles O2 to moles CO2, convert moles CO2 to mL.
Post your work if you get stuck.
The equation for burning C2H2 is
2C2H2(g) + 5O2(g) ⎯→ 4CO2(g) + 2H2O(g)
a. If 15.9 L C2H2 react at STP, how many
moles of CO2 are produced? (Hint: At
STP, 1 mol = 22.41 L for any gas.)
b. How many milliliters of CO2 (density =
1.977 g/L) can be made when 59.3 mL O2
(density = 1.429 g/L) react?
3 answers
2.39
Write and balance the proper reaction for ethyne (C2H2) being burned in an oxygen atmosphere.
a. If 15.9 L C2H2 react at standard temperature and pressure, how many moles of CO2 are produced?
b. How many milliliters of CO2 (density = 1.977 g/L) can be made when 59.3 mL O2 (density = 1.429 g/L) react?
a. If 15.9 L C2H2 react at standard temperature and pressure, how many moles of CO2 are produced?
b. How many milliliters of CO2 (density = 1.977 g/L) can be made when 59.3 mL O2 (density = 1.429 g/L) react?
1 answer