The following volume of reagents were used: A = 20.0 ml (Density = 1.04 g/cm3) B = 10.0 ml (Density = 0.79 g/cm3) Calculate the limiting reagent. Calculate the theoretical yield of compound C. Calculate the percentage yield if you obtained 18.1 g of compound C experimentally.

The following volume of reagents were used: A = 20.0 ml (Density = 1.04 g/cm3) B = 10.0 ml (Density = 0.79 g/cm3) Calculate the limiting reagent. Calculate the theoretical yield of compound C. Calculate the percentage yield if you obtained 18.1 g of compound C experimentally.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Determine the theoretical mass of aspirin (acetyl salicylic acid) when using 3.682 grams of…

A: Salicylic acid reacts with acetic anhydride to give aspirin or acetylsalicylic acid and acetic acid.…

Q: KOH (aq) + H3PO4 (aq) → K3PO4 (aq) + 3 H2O (l) In this reaction, 25.800 g of KOH…

Q: If 3.29 g Cu(NO3)2 are obtained from allowing 2.05 g of Cu to react with excess HNO3: Part A What is…

Q: Compound A reacts with Compound B to form only one product, Compound C, and it's known the usual…

A: The given reaction is: A + B -------> C Percent yield = 95% Mass of A =4.5 g Mass of product…

Q: Suppose 2.5 g of Compound A and 3.0 g of Compound B are consumed in a reaction that produces only…

A: According to law of conservation of mass, mass of products is equal to mass of reactants

Q: A3.82-g sample of magnesium nitride is reacted with 7.73 g of water. Mg3N2 + 3H20 - 2NH3 + 3M9O The…

A: This problem can be solved through calculation of liming reagent.

Q: Consider the harber-bosch process for the synthesis of ammonia from its elements. Calculate the…

A: The given chemical reaction as follows,N2(g)+3H2(g)⇌2NH3(g)amount of H2 for reaction =15.6 gramand…

Q: 2Mg(s)+O2(g)→2MgO(s)2Mg(s)+O2(g)→2MgO(s) When 13.2 gg MgMg reacts with 14.0 gg O2O2, 12.3 gg MgOMgO…

Q: When gaseous nitrogen and gaseous hydrogen are reacted at high temperatures in the presence of a…

A: The reaction in the problem is the formation of ammonia from nitrogen and hydrogen.…

Q: The limiting reagent is

Q: Take the reaction: NH3 + O2 ---> NO + H2O. In an experiment, 3.25 g of NH3 are allowed to react with…

Q: hen 8.00 g of Aluminum is allowed to react with 35.0 g of chlorine gas to produce aluminum chloride,…

A: The limiting reagent in a chemical reaction is a reactant that is totally consumed when the chemical…

Q: This question will walk you through the steps of determining which reactant is limiting based on a…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water. Mg3N2 + 3H20 –→ 2NH3 + 3M9O…

Q: The theoretical yield of a product in a reaction is determined by the limiting reactant. O True…

A: 1.Theoretical Yield is the amount of product formed from a given balanced equation. 2. Actual yield…

Q: "A liquid fuel mixture contains 30.25% hexane (C6H14), 17.10% heptane (C7H16), and the rest octane…

A: Mass of fuel mixture = 15 kgHexane = 30.25%Heptane = 17.10%Octane = 100 - (30.25+17.10)…

Q: Adipic acid, H2C6H&O4, used to produce nylon, is made commercially by a following reaction petween…

A: the given reaction is 2C6H12+5O2→2H2C6H8O4+2H2O According to the above reaction 2 mole of…

Q: DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: 2C6H5…

Q: Use only 1 decimal point for atomic masses. Determine the yield (amount of product) of CH4(g) if…

A: Number of moles of Ni3C is calculated as given below,

Q: Boron trichloride is prepared from the following reaction:…

A: Mass of B2O3 = 3.387 g Mass of Cl2 = 9.504 g Mass of C = 2.509 g We need to find limiting…

Q: How many grams of H₂ can be formed from 54.6 grams of NH₃ in the following reaction? 2 NH₃(g) → 3…

A: Given that the mass of ammonia is 54.6 g which decomposes to form nitrogen gas and hydrogen gas. The…

Q: Consider the reaction of solid PbO and gaseous NH3 to form solid Pb, nitrogen gas, and water vapor.…

A: The balanced chemical reaction of solid PbO and gaseous NH3 to formsolid Pb, nitrogen gas and water…

Q: Fe,03 + HCI → FeCl, + H2O 5 g 5 g ?g 5. How many grams of the product is produced?

Q: 1.05 gg H2H2 is allowed to react with 10.3 gg N2N2, producing 1.09 gg NH3NH3. Part A What is the…

A: For this question, first calculate moles for both reactant. Then use mol to mol ratio for reactant…

Q: H2CO + HCOOH +HCN >H5C3O3N There are three reagents in this reaction If you have 30.7 grams of…

A: Given: mass of H2CO = 30.7 grams mass of HCOOH = 46.0 grams mass of HCN = 24.1 grams molar mass of…

Q: Enter your answer in the provided box. Diethyl ether is produced from ethanol according to the…

Q: The reaction of 35.0 g of Al with 44.1 g of Cr₂O₃ produced 13.0 g of Cr. 2Al + Cr₂O₃ ⟶ Al₂O₃ + 2Cr…

A: The balanced reaction taking place is given as, => 2 Al + Cr2O3 → Al2O3 + 2 Cr Given: Mass of…

Q: Calculate the percent yield for water.

A: Number of moles = mass/molar mass Molar mass of WO3 is 231.838 g/mol Percent yield = (actual…

Q: produced (in other words, what is the theoretical yield)? Only write the number with correct sig…

A: Molar mass of NaHCO3 = 84.01 g Molar mass of Na2CO3 = 105.99 g From balanced reaction, 2×84.01 g…

Q: Consider the reaction: C2H4(g) + 302 (g) – 2C02 (g) + 2H20(g) If 23.21 g of C2H4(g) react with…

A: The balanced Chemical Reaction is - C2H4(g) + 3O2(g) ----> 2CO2(g) + 2H2O(g) The molar masses of…

Q: A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water. Mg3N2 + 3H20 → 2NH3 + 3M9O The…

A: To Solve this first we have to calculate the limiting reactant then theoretical yield of MgO is…

Q: Calculate the maximum amount in grams of H₂O that can be produced by the reaction of 550 mg of H₂…

A: Given, H2(g) + O2(g) ➝ H2O(g) Balancing the above equation: 2H2(g) + O2(g) ➝ 2H2O(g) Note: 1000 mg =…

Q: A chemist was able to produce 27.9 grams of phosphorus tribromide from 35.0 grams of bromine. What…

Q: 2KHC4H406 + Na2C03 H20 + 6 H20→2 KNAC4H406.4 H20 + co21 Balanced Chemical Reaction % Composition by…

A: Interpretation - To determine the % composition by mass of each compound for this given reaction -…

Q: .) Consider the following reaction. 3H2(g) + WO3(s) → 3H2O(g) + W(s) When 500.0 g of WO3(s) react…

A: Since you have posted multiple questions,we will solve first question for you. To get remaining…

Q: consider the following balanced equation. N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) Determine the…

A: Given, N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) Given, mass of N2O4 react = 60.0 g mass of N2H4…

Q: A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water.…

A: The balanced reaction taking place is given as, => Mg3N2 + 3 H2O → 2 NH3 + 3 MgO Given: Mass of…

Q: Methyl salicylate (C₂H8O3) (density = 1.18 g/mL) is dissolved in 100 mL of 6.0 M NaOH, and heated…

A: Theoretical is defined as the maximum amount of the product that can be formed in a given chemical…

Q: For the following reaction, 4.42 grams of carbon disulfide are mixed with excess chlorine gas. The…

Q: Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) →…

A: Given - Un - Balanced Chemical equation is - C₁₂H₂₂O₁₁(s) + O₂(g) → CO₂(g) + H₂O(l) The balanced…

Q: (CH₂(CH₂) CH₂) reacts with gaseous oxygen gas (0₂) to produce gaseous carbon dioxide (CO₂) and…

A: we have to calculate the percentage yield of water

Q: Use 1 decimal point for all atomic masses. 82.1 g of Ni3C(s) are reacted with 1.80 g of H2(g) by the…

A: The given reaction is shown below.

Q: Sodium chloride is formed from the reaction between sodium metal and chlorine gas. 2 Na + Clk → 2…

A: Q1) (a) 2Na + Cl2 ----------> 2 NaCl 2…

Q: 2Cu20(s) + Cu2S(s)→ 6Cu(s) + SO2(g) a) If 12.87 kg of the copper (1) oxide ore and 11.921 kg of…

Q: A student uses 0.40 mL of bromobenzene and 0.052 g of elemental magnesium for their Unit 6…

A: Answer is explained below.

Q: Compound A reacts with Compound B to form only one product, Compound C, and it's known the usual…

A: Given,when A reacts with B to form only one product C,mass of A = 1.0 gthe produced mass of C =3.7…

Question

The following volume of reagents were used: A = 20.0 ml (Density = 1.04 g/cm3)
B = 10.0 ml (Density = 0.79 g/cm3)

Calculate the limiting reagent.

Calculate the theoretical yield of compound C.
Calculate the percentage yield if you obtained 18.1 g of compound C experimentally.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step by step

Solved in 4 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

20
In the complete combustion of liquid octane, 2 C3H18 (1) + 25 O2 (g) --> 16 CO2 (g) + 18 H2O (g) determine the mass in grams of carbon dioxide produced if 12.2 grams of octane are used.
One method to extract copper metal, Cu, from its ores is as follows: Cu₂S (s) + 2 Cu₂O (s) – 6 Cu (s) + SO2 (g) If the theoretical yield from this reaction is 3.451 g of Cu and the actual yield is 1.243 g of copper, Cu, what is the percentage yield of Cu for this reaction? Percent yield of Cu = Number %
1.41 gg H2H2 is allowed to react with 10.5 gg N2N2, producing 1.36 gg NH3NH3. Part A What is the theoretical yield in grams for this reaction under the given conditions, What is the percent yield for this reaction under the given conditions? Express your answer to three significant figures and include the appropriate units.
You are given a mixture of CuCO3 and CuO. You place the mixture in a crucible and heat it to decompose the CuCO3 into CO2 gas and CuO. You made sure that the CuCO3 had completely decomposed by constantly heating it, cooling it, and weighing it until the mass remains the same. Using the data below from the experiment, calculate the % CuCO3 in the original sample. Mass of empty crucible: 22.19 g Mass of crucible + sample before heating: 23.193 g Mass of crucible + sample at constant mass: 22.851 g PLease show and create one solution map: i made this solution map, is it correct? 1.561g CO2 x (1mol CO2/44.01g CO2) x (1mol CrCO3/1mol CO2) x (112.01g CrCO3/1mol CrCO3)= 3.973g CrCO3 than, (3.973/25.422) x 100% = 15.63% 2.) A 12.622 g sample of a compound that contains sulfur is analyzed by precipitating all the sulfur as BaSO4. If 11.957 g of BaSO4 are obtained in the analysis, what is the percentage of sulfur in the original compound? (Need help with this one too)
Compound A reacts with Compound B to form only one product, Compound C, and it's known the usual percent yield of C in this reaction is 86.%. Suppose 6.0 g of A are reacted with excess Compound B, and 6.5 g of Compound C are successfully isolated at the end of the reaction. What was the theoretical yield of C? Round your answer to the nearest 0.1 g. How much B was consumed by the reaction? Round your answer to the nearest 0.1 g. 1 x10 ロ・ロ X μ 010 Ś
You set out to synthesize aspirin (C9H8O4) and begin with 5.0 grams of salicylic acid (C7H6O3) and 5.0 grams of acetic anhydride (C4H6O3). You are able to only make 10.0 mg of aspirin, what is your percent yield? C7H6O3(aq) + C4H6O3(aq) →C9H8O4(aq) + CH3COOH (aq)
The combustion of propane occurs through the following chemical reaction. C3 H3 (g) + 5 O2 (g). - 3 CO2 (g) + 4 H,O (g) -> How many grams of H20 can be made by reacting 11.27 grams of oxygen gas?
n the reaction of 1.88 g of salicylic acid (MM = 138.122 g/mol) with 1.09 g of acetic anhydride (MM = 102.089 g/mol) a student obtained 1.16 g of acetylsalicylic acid (MM = 180.159 g/mol). What is the percent yield? Report your answer to 1 decimal place and only report the numerical value (no units).
If 5.45 g of potassium chlorate are decomposed to form potassium chloride, 1.75 g of oxygen gas are also given off. Find the percent yields. - 2 KCIO3 → 2 KCI + 3 02 Please remember significant figures in your answer! Units not required.
8.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 128. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured. Use this information to find the molecular formula of X
What mass of H2O is produced from 100 g of H2 in the foillowing reaction. 2H2 + O2 → 2H2O