Directions: Write T if the statement is true and F it is false. Place your answers on the blank provided in each number. 1. Chemists need a measurement called percent yield to indicate how successful a reaction has been. _2. The theoretical yield is the ratio of the actual yield to the theoretical yield, expressed as a percentage. 3. The actual yield is the amount of product that is actually formed when the reaction is carried out in the laboratory. 4. The maximum amount of product that could be formed from the given amounts of reactants is called the percent yield.

Directions: Write T if the statement is true and F it is false. Place your answers on the blank provided in each number. 1. Chemists need a measurement called percent yield to indicate how successful a reaction has been. _2. The theoretical yield is the ratio of the actual yield to the theoretical yield, expressed as a percentage. 3. The actual yield is the amount of product that is actually formed when the reaction is carried out in the laboratory. 4. The maximum amount of product that could be formed from the given amounts of reactants is called the percent yield.

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

Similar questions

Chromium(III) ions are very poisonous. They can be removed from solution by precipitating very insouble chromium(III) hydroxide. Chromium(III) chloride reacts with calcium hydroxide to form chromium(III) hydroxide and calcium chloride. Write the balanced formula unit equation for the reaction stated above. Now, determine the total ionic equation for the reaction stated above. Now write the balanced net ionic equation for the reaction stated above.
1. Consider the generic reaction: A + 2B→ CHow many moles of C are formed upon the complete reaction of:A. 5.0 moles of AB. 5.0 moles of B 2. For the reaction: 2N2O5 → 4NO2 + O2Calculate how many moles of NO2 form when each amount of the reactant completely reacts.A. 1.3 moles N2O5B. 1.006x10-3 mole N2O5 3. For the reaction: 2S + 3O2 → 2SO3A. Calculate the moles of S needed to completely react with 1.75 moles of O2B. Calculate the moles of product that form when 1.75 moles of O2 completely reacts. Assume thereis more than enough S. 4. For the reaction: 2S + 3O2 → 2SO3A. Calculate the mass of S (32.07 g/mol) needed to completely react with 5.3 g of O2 (32.00 g/mol).B. Calculate the mass of SO3 (80.07 g/mol) that form when 5.3 g of O2 completely reacts. Assumethere is more than enough S. 5. A mixture containing 21 moles of F2 and 8 moles of S is allowed to react according to the reaction:3F2 + S → SF6A. What is the limiting reactant?B. How many moles of the excess reactant remain after…
Suppose from experimental results, the actual yield of HCl is 43.7 g whereas the calculated theoretical yield is 56.0g. What would be the percent yield of HCl? A. 78.04% HCl B. 28.65 % HCl C. 57.30 % HCl D. 20.02 % HCl E. 61.93 % HCl
Balance the reaction. note: Add four numbers.__________ C7H14 + __________ O2 → ______________ CO2 + ___________ H2O What type of reaction is this? ______________
11. An old bike is left abandoned in a shed for many years, where it begins to rust. The bike is not exposed to rain or wind that would cause the rust to fall off the bike. Is the bike gaining mass, losing mass, or maintaining the same mass as it rusts? Explain. 12. Describe 2 factors that can reduce percent yield when a scientist is trying to create a specific chemical product. Explain specifically how each factor reduces percent yield. 13. How did decomposition reactions help early chemists come to the Law of Definite Proportions?
1. List the following carbocations from least stable to most stable? + ő őt tá CH'S CH13 2. Which alkene product do you expect to be the major product? Explain based on the mechanism and the product stability.
If a reaction is run that is supposed to produce 125 g (theoretical yield) of product and the actual yield of product that was produced was 73.5 g, what is the percent of yield of this reaction? A. 170% B. 1.70% C. 73.5% D. 58.8%
Write the balanced equation for the following situation. In addition, list the reaction type. You must tell the amount of every substance that remains in the container at the end of the reaction. Assume that all reactions go to completion. If only stoichiometry, tell how much excess reactant is used. Reaction Type:a. Combination Reactionb. Decomposition Reactionc. Single Displacement / THIS IS ONE TYPE OF Oxidation Reduction Reaction d. Precipitation Reactione. Gaseous Reactionf. Neutralization Reactiong. Combustion Reaction 61.802 cg of nitrogen gas is reacted with 61.802 cg of hydrogen gas to form ammonia
1. Write the correct chemical equation for the following reaction: when beryllium chloride reacts with silver (I) nitrate, beryllium nitrate and silver (I) chloride are formed 2. Write the correct skeleton equation for the following: fluorine gas reacts with calcium metal to form solid calcium fluoride
Balance the reaction. note: Add four numbers.___________ Fe(OH)3 + _________ H2SO4 → ________ Fe2(SO4)3 + ________ H2O
Balance the following chemical equation by placing a coefficient (including 1) in each answer box that is in front of each reactant and each product. While coefficients that are equal to 1 are not placed in front of either a reactant or product, you MUST include any coefficient that is equal to 1 in this problem. type your answer... Re3P7- type your answer... Re + type your answer... P4
Please answer all parts of this question. 1. Magnesium oxide can be made by heating magnesium metal in the presence of oxygen gas. a. Write the balanced equation, including phase symbols. b. When 10.1 g of magnesium reacts with 10.5 g of oxygen gas, 11.9g of magnesium oxide is collected. i. Determine the limiting reactant ii. Determine the theoretical yield iii. Determine the percent yield for the reaction