Question

In: Chemistry

the reaction of 7.26 g of carbon with excess O2 yeilds 8.20 g of CO2. What...

the reaction of 7.26 g of carbon with excess O2 yeilds 8.20 g of CO2. What is the percent yeild of the reaction?

Solutions

Expert Solution

  C           +         O2      ----------->          CO2

1 mol                                                     1 mol

= 12 g                                                     = 44 g

In the above balanced equation,

          12g of carbon with excess O2 produced   44g of CO2

So, 7.26 g of carbon with excess O2 will produce ? g of CO2.

         ? = (7.26 g of carbon/12 g of carbon) x 44g of CO2

            = 26.62 g   CO2

7.26 g of carbon with excess O2 will produce 26.62 g of CO2. (This is called theoretical yield)

But it is given that 7.26 g of carbon with excess O2 yeilds 8.20 g of CO2. (This is called actual yield)

Percent yield = (actual yield / theoretical yield) x 100

                       = (8.20 g CO2 / 26.62 g CO2) X 100

                      = 30.80 %

Percent yield = 30.80 %

Therefore, percent yield of the reaction = 30.80 %

queen_honey_blossom answered 3 months ago
Next > < Previous

Related Solutions

The combustion reaction of propane is as follows. C3H8(g) + 5 O2(g) → 3 CO2(g) +...
The combustion reaction of propane is as follows. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. Answer in KJ/mol reaction (1):     C(s) + O2(g) → CO2(g)     ΔH = −393.5 kJ/mol reaction (2):     H2(g) + 1/2 O2(g) → H2O(l)     ΔH = −285.8 kJ/mol reaction (3):     3 C(s) + 4 H2(g) → C3H8(g)     ΔH = −103.8 kJ/mol
A mixture of CS2(g) and excess O2(g) is placed in a 10 L reaction vessel at...
A mixture of CS2(g) and excess O2(g) is placed in a 10 L reaction vessel at 100.0 ∘C and a pressure of 3.10 atm . A spark causes the CS2 to ignite, burning it completely, according to the equation: CS2(g)+3O2(g)→CO2(g)+2SO2(g) After reaction, the temperature returns to 100.0 ∘C, and the mixture of product gases (CO2, SO2, and unreacted O2) is found to have a pressure of 2.50 atm . What is the partial pressure of each gas in the product...
A mixture of CS2(g) and excess O2(g) is placed in a 10 L reaction vessel at...
A mixture of CS2(g) and excess O2(g) is placed in a 10 L reaction vessel at 100.0 ∘C and a pressure of 3.10 atm . A spark causes the CS2 to ignite, burning it completely, according to the equation: CS2(g)+3O2(g)→CO2(g)+2SO2(g) After reaction, the temperature returns to 100.0 ∘C, and the mixture of product gases (CO2, SO2, and unreacted O2) is found to have a pressure of 2.50 atm . What is the partial pressure of each gas in the product...
A 2.00 L reaction container at 25.0 °C contains CO2 (g) and O2 (g). The total...
A 2.00 L reaction container at 25.0 °C contains CO2 (g) and O2 (g). The total pressure of the gases in the container was 656 torr and the mole fraction of CO2 is 0.245. Calculate the partial pressure of oxygen gas in the mixture Calculate the mass of oxygen gas in the mixture (in g). Which gas will rise to the top of the container? Explain your answer. Calculate the total volume of the container if 15.0 g of helium...
Balance the combustion reaction of chrysene (C18H12) at 298K. C18H12(s)+ O2(g) CO2(g) + H2O(l) What is...
Balance the combustion reaction of chrysene (C18H12) at 298K. C18H12(s)+ O2(g) CO2(g) + H2O(l) What is the value of ng for the combustion reaction? ng = mol What is Hcomb of chrysene if Ecomb = -8942.6 kJ/mol? Hcomb = kJ/mol What is the heat of formation of chrysene? See Thermodynamic Properties Hf = kJ/mol
Consider this reaction between solid carbon and carbon dioxide gas. C(s) + CO2(g) ⇌ 2 CO(g);...
Consider this reaction between solid carbon and carbon dioxide gas. C(s) + CO2(g) ⇌ 2 CO(g); ΔH = +172.5 kJ/mol Please explain the following: When chemical systems are subjected to stresses, the equilibrium position may shift toward the reactants or products, or it may be unaffected. How would each of the following changes affect this equilibrium? 1. decreasing the temp 2. increasing the CO2 3. increasing the volume of the container 4. adding C 5. adding a catlyst Options: Would...
Consider the reaction: 2 CO2(g) + Heat = 2 CO(g) + O2(g) 1.  Predict the effect on...
Consider the reaction: 2 CO2(g) + Heat = 2 CO(g) + O2(g) 1.  Predict the effect on the equilibrium system if the reaction temperature is decreased. (You may wish to write the equilibrium constant expression for the reaction first). a) The equilibrium will shift to the right favoring the products. b) The equilibrium will shift to the side that the light side of the force is on. c) There will be no effect. d) The equilibrium will shift to the left...
Question 2 options: For the reaction  CH4 + O2 →CO2 + H2OCH4 + O2 →CO2 + H2O...
Question 2 options: For the reaction  CH4 + O2 →CO2 + H2OCH4 + O2 →CO2 + H2O what are the coefficients for each reactant or product? a. CH4 b. O2 c. CO2 d. H2O Question 3 (2 points) Question 3 options: For the reaction  NaOH + AlCl3 →NaCl + Al(OH)3NaOH + AlCl3 →NaCl + Al(OH) what are the coefficients for each reactant or product? a. NaOH b. AlCl3 c. NaCl d. Al(OH)3 Question 4 (2 points) Question 4 options: For the reaction  H2O2...
When propane is burned, the balanced reaction is: C3H8(l) + 5 O2(g) -> 3 CO2(g) +...
When propane is burned, the balanced reaction is: C3H8(l) + 5 O2(g) -> 3 CO2(g) + 4 H2O(g). If 31.66 L of water vapor are produced at 865.7 torr and 75°C, how many grams of propane were burned?
Consider the following equilibrium. CS2(g) + 3 O2(g) equilibrium reaction arrow CO2(g) + 2 SO2(g) If...
Consider the following equilibrium. CS2(g) + 3 O2(g) equilibrium reaction arrow CO2(g) + 2 SO2(g) If the reaction is started in a container with 5.59 atm CS2 and 13.3 atm O2, what is Kp if the partial pressure of CO2 is 3.76 atm at equilibrium? (There is no change in temperature and the initial partial pressures of the products are equal to 0.)
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT