Question

Determine the theoretical yield of CO2 (in grams) for the reaction below if you have 18.0...

Determine the theoretical yield of CO2 (in grams) for the reaction below if you have 18.0 g of C2H4 and 45.0 g of O2.

C2H4(g) + 3 O2(g)à2 CO2(g) + 2 H2O(l)

Homework Answers

Answer #1

moles of C2H4 = mass / molar mass = 18.0 g / 28.0532 g/mol = 0.6416 mol

moles of O2 = 45 g/ 32 g/mol = 1.40 mol

from the balanced equation

1 mole of C2H4 required 3 moles of O2 accordingly

0.6416 mol required 3 x 0.6416 = 1.9248 mol O2

but we have 1.40 mol

so limiting agent is C2H4

from balanced equation

1 mol of C2H4 will produce 2 mol of CO2 accordingly

0.6416 mol produces 2 x 0.6416 mol = 1.2832 moles of CO2

theritcal mass of CO2 = 1.2832 mol x 44 g/mol = 56.4608 grams

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
C6H6 + O2  →  CO2 + H2O If at the beginning of the reaction you used 9.92 g...
C6H6 + O2  →  CO2 + H2O If at the beginning of the reaction you used 9.92 g C6H6 and 9.85 g O2, what is the theoretical yield (in grams) of H2O? (you will need to find the limiting reagent and then the theoretical yield of H2O from this reagent)
For the balanced equation shown below, if the reaction of 40.8 grams of C6H6O3 produces a...
For the balanced equation shown below, if the reaction of 40.8 grams of C6H6O3 produces a 39.0% yield, what is the theoretical yield and how many grams of H2O would be produced? (C = 12.01 amu, H = 1.01 amu, O = 16.00 amu) C6H6O3 + 6 O2 → 6 CO2 + 3 H2O Theoretical yield = Blank 1 grams of H2O Actual yield = Blank 2 grams of H2O
Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18...
Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
Find the ΔH and ΔE for the reaction below: C2H6(g) + 7/2 O2(g) à 2 CO2(g)...
Find the ΔH and ΔE for the reaction below: C2H6(g) + 7/2 O2(g) à 2 CO2(g) + 3 H2O (l) given the following data: ΔHf C2H6 = -84.7 kJ/mol                  ΔHf CO2 = -393.5 kJ/mol ΔHf H2O = -286 kJ/mol
Determine the theoretical yield (in grams) of AlBr3 when 5.00 grams of Al and excess Br2...
Determine the theoretical yield (in grams) of AlBr3 when 5.00 grams of Al and excess Br2 are reacted according to the reaction below. Molar mass of AlBr3 is 266.68 g/mol. 2Al(s) + 3Br2(l) ⟶ 2AlBr3(s)
What is the percent yield of CO2 if 42.24 g of CO2 are formed from the...
What is the percent yield of CO2 if 42.24 g of CO2 are formed from the reaction of 4.00 moles of C8H18 with 8.00 moles of O2 according to the balanced equation below? 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(g)
Consider the balanced chemical reaction shown below. 2 C3H6(g) + 9 O2(g) 6 CO2(g) + 6...
Consider the balanced chemical reaction shown below. 2 C3H6(g) + 9 O2(g) 6 CO2(g) + 6 H2O(l) In a certain experiment, 6.004 g of C3H6(g) reacts with 2.118 g of O2(g). (a) Which is the limiting reactant? _____ is the limiting reactant. (b) How many grams of CO2(g) form? _____g of CO2(g) form. (c) How many grams of H2O(l) form? _____g of H2O(l) form. (d) How many grams of the excess reactant remains after the limiting reactant is completely consumed?_____...
What is the theoretical yield (in grams) of acetic acid, HC2H3O2, when 8.925 g of carbon...
What is the theoretical yield (in grams) of acetic acid, HC2H3O2, when 8.925 g of carbon dioxide reacts with 1.735 g of hydrogen according to the following reaction: 2 CO2 (g) + 4 H2 (g) → HC2H3O2 (g) + 2 H2O (g) Use the correct number of significant figures.
Use the enthalpy data below to determine the standard reaction enthalpy ∆h0r for the reaction: C6H14...
Use the enthalpy data below to determine the standard reaction enthalpy ∆h0r for the reaction: C6H14 (g) + 9.5 O2 (g) = 6 CO2 (g) + 7 H2O (g) Data: C6H14 (l) + 9.5 O2 (g) = 6 CO2 (g) + 7 H2O (l): ∆h0r = −1791 BTU / lb-mol Justify your answer clearly.
(a) Consider the combustion of ethylene, given below. C2H4(g) + 3 O2(g) ? 2 CO2 (g)...
(a) Consider the combustion of ethylene, given below. C2H4(g) + 3 O2(g) ? 2 CO2 (g) + 2 H2O (g) If the concentration of C2H4 is decreasing at the rate of 0.26 M/s, what are the rates of change in the concentrations of CO2 and H2O? CO2 (b) The rate of decrease in N2H4 partial pressure in a closed reaction vessel from the following reaction is 41 torr/hr. N2H4 (g) + H2 (g) ? 2 NH3 (g) What are the...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT