Theoretical yield of S O 2 has to be given for the chemical reaction where sulfur dioxide is produced from sulfur and oxygen where, 9.75 g of S O 2 is only obtained out of the possible 11.2 g . Concept Introduction: In a chemical reaction, when the reactants gives product, the amount of product formed from the given amount of reactant can be said in terms of yield. Theoretical yield of a chemical reaction is the maximum amount of the product that can be obtained from the given amount of reactants provided there is no loss or inefficiencies occur. The actual yield of the chemical reaction is the experimental yield that is obtained. Actual yield of the product is always lesser than the theoretical yield. For this, there are two reasons. They are, In mechanical process, some of the product is lost. Mechanical process involves the transfer of materials from a container to another container. Unwanted side reactions occur in the actual chemical reaction due to impurities present. These are not considered in theoretical yield. Actual yield is the amount of product that is got from a chemical reaction. The actual yield has to be measured and not calculated. Percent yield is the term that is used to tell about the product loss. It is the ratio of the actual amount of product that is obtained in a chemical reaction to the theoretical yield multiplied by 100 to give percent. Mathematical equation for percent yield is given as, P e r c e n t y i e l d = Actual yield Theoretical yield x 100

Question

5 What would the complete ionic reaction be if aqueous solutions of potassium sulfate and barium acetate were mixed? ed of Select one: O a 2 K SO4 + Ba2 +2 C₂H3O21 K+SO4 + Ba2+ + 2 C2H3O21 K+SO42 + Ba2 +2 C2H3O2 BaSO4 +2 K+ + 2 C2H3O estion Ob. O c. Od. 2 K SO4 +Ba2 +2 C₂H₂O₂ BaSO4 + K+ + 2 C2H3O BaSO4 + K + 2 C2H301 →Ba² +SO42 +2 KC2H3O s page

Answer 1

Question

Chapter 6, Problem 6.83EP

(a)

Interpretation Introduction

Interpretation:

Theoretical yield of SO2 has to be given for the chemical reaction where sulfur dioxide is produced from sulfur and oxygen where, 9.75 g of SO2 is only obtained out of the possible 11.2 g.

Concept Introduction:

In a chemical reaction, when the reactants gives product, the amount of product formed from the given amount of reactant can be said in terms of yield.

Theoretical yield of a chemical reaction is the maximum amount of the product that can be obtained from the given amount of reactants provided there is no loss or inefficiencies occur. The actual yield of the chemical reaction is the experimental yield that is obtained. Actual yield of the product is always lesser than the theoretical yield. For this, there are two reasons. They are,

In mechanical process, some of the product is lost. Mechanical process involves the transfer of materials from a container to another container.

Unwanted side reactions occur in the actual chemical reaction due to impurities present. These are not considered in theoretical yield.

Actual yield is the amount of product that is got from a chemical reaction. The actual yield has to be measured and not calculated.

Percent yield is the term that is used to tell about the product loss. It is the ratio of the actual amount of product that is obtained in a chemical reaction to the theoretical yield multiplied by 100 to give percent. Mathematical equation for percent yield is given as,

Percent yield = Actual yieldTheoretical yield x 100

(b)

Interpretation Introduction

Interpretation:

Actual yield of SO2 has to be given for the chemical reaction where sulfur dioxide is produced from sulfur and oxygen where, 9.75 g of SO2 is only obtained out of the possible 11.2 g.

Concept Introduction:

In a chemical reaction, when the reactants gives product, the amount of product formed from the given amount of reactant can be said in terms of yield.

Theoretical yield of a chemical reaction is the maximum amount of the product that can be obtained from the given amount of reactants provided there is no loss or inefficiencies occur. The actual yield of the chemical reaction is the experimental yield that is obtained. Actual yield of the product is always lesser than the theoretical yield. For this, there are two reasons. They are,

In mechanical process, some of the product is lost. Mechanical process involves the transfer of materials from a container to another container.

Unwanted side reactions occur in the actual chemical reaction due to impurities present. These are not considered in theoretical yield.

Actual yield is the amount of product that is got from a chemical reaction. The actual yield has to be measured and not calculated.

Percent yield is the term that is used to tell about the product loss. It is the ratio of the actual amount of product that is obtained in a chemical reaction to the theoretical yield multiplied by 100 to give percent. Mathematical equation for percent yield is given as,

Percent yield = Actual yieldTheoretical yield x 100

(c)

Interpretation Introduction

Interpretation:

Percent yield of SO2 has to be given for the chemical reaction where sulfur dioxide is produced from sulfur and oxygen where, 9.75 g of SO2 is only obtained out of the possible 11.2 g.

Concept Introduction:

In a chemical reaction, when the reactants gives product, the amount of product formed from the given amount of reactant can be said in terms of yield.

Theoretical yield of a chemical reaction is the maximum amount of the product that can be obtained from the given amount of reactants provided there is no loss or inefficiencies occur. The actual yield of the chemical reaction is the experimental yield that is obtained. Actual yield of the product is always lesser than the theoretical yield. For this, there are two reasons. They are,

In mechanical process, some of the product is lost. Mechanical process involves the transfer of materials from a container to another container.

Unwanted side reactions occur in the actual chemical reaction due to impurities present. These are not considered in theoretical yield.

Actual yield is the amount of product that is got from a chemical reaction. The actual yield has to be measured and not calculated.

Percent yield is the term that is used to tell about the product loss. It is the ratio of the actual amount of product that is obtained in a chemical reaction to the theoretical yield multiplied by 100 to give percent. Mathematical equation for percent yield is given as,

Percent yield = Actual yieldTheoretical yield x 100

Expert Solution & Answer

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

Students have asked these similar questions

5 What would the complete ionic reaction be if aqueous solutions of potassium sulfate and barium acetate were mixed? ed of Select one: O a 2 K SO4 + Ba2 +2 C₂H3O21 K+SO4 + Ba2+ + 2 C2H3O21 K+SO42 + Ba2 +2 C2H3O2 BaSO4 +2 K+ + 2 C2H3O estion Ob. O c. Od. 2 K SO4 +Ba2 +2 C₂H₂O₂ BaSO4 + K+ + 2 C2H3O BaSO4 + K + 2 C2H301 →Ba² +SO42 +2 KC2H3O s page

(28 pts.) 7. Propose a synthesis for each of the following transformations. You must include the reagents and product(s) for each step to receive full credit. The number of steps is provided. (OC 4) 4 steps 4 steps OH b.

LTS Solid: AT=Te-Ti Trial 1 Trial 2 Trial 3 Average ΔΗ Mass water, g 24.096 23.976 23.975 Moles of solid, mol 0.01763 001767 0101781 Temp. change, °C 2.9°C 11700 2.0°C Heat of reaction, J -292.37J -170.473 -193.26J AH, kJ/mole 16.58K 9.647 kJ 10.85 kr 16.58K59.64701 KJ mol 12.35k Minimum AS, J/mol K 41.582 mol-k Remember: q = mCsAT (m = mass of water, Cs=4.184J/g°C) & qsin =-qrxn & Show your calculations for: AH in J and then in kJ/mole for Trial 1: qa (24.0969)(4.1845/g) (-2.9°C)=-292.37J qsin = qrxn = 292.35 292.37J AH in J = 292.375 0.2923kJ 0.01763m01 =1.65×107 AH in kJ/mol = = 16.58K 0.01763mol mol qrx Minimum AS in J/mol K (Hint: use the average initial temperature of the three trials, con Kelvin.) AS=AHIT (1.65×10(9.64×103) + (1.0 Jimai