Chemistry for Today
8th Edition
ISBN: 9781133606994
Author: Seager, Spencer L./
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
error_outline
This textbook solution is under construction.
Students have asked these similar questions
How would the following errors affect the empirical formula for the compound?
The student ran out of time and did not do the second heating. Explain how this error will affect the calculation for the number of moles of water in the hydrate? Will the final answer be artificially high or low? How do you know?
The student recorded the mass of the cup + sample incorrectly and started with 2.2 g of hydrated compound but used 2.0 g in the calculations. Explain how this error will affect the calculation for the number of moles of water in the hydrate? Will the final answer be artificially high or low? How do you know?
The approximate molar mass of a volatile liquid can be determined by:1. Heating a sample of the liquid in a flask with a tiny hole at the top, which converts the liquid into gas that may escape through the hole2. Removing the flask from heat at the instant when the last bit of liquid becomes gas, at which time the flask will be filled with only gaseous sample at ambient pressure3. Sealing the flask and permitting the gaseous sample to condense to liquid, and then weighing the flask to determine the sample’s mass as shown.
How would the following errors affect the empirical formula for the compound? That is, will these errors cause the calculated number of moles of water in the hydrate to be artificially high or low?
a. The student ran out of time and did not do the second heating. Explain how this error will affect the calculation for the number of moles of water in the hydrate? Will the final answer be artificially high or low?
Knowledge Booster
Similar questions
- Can the subscripts in a chemical formula be fractions? Explain.arrow_forwardhat do the coefficients of a balanced chemical equation tell us about the proportions in which atoms and molecules react on an individual (microscopic) basis?arrow_forwardWithout consulting your textbook, list and explain the main postulates of the kinetic molecular theory for gases. How do these postulates help us account for the following bulk properties of a gas: the pressure of the gas and why the pressure of the gas increases with increased temperature; the fact that a gas tills its entire container; and the fact that the volume of a given sample of gas increases as its temperature is increased.arrow_forward
- Is there a difference between a homogeneous mixture of hydrogen and oxygen in a 2:1 ratio and a sample of water vapor? Explain.arrow_forwardDescribe any visual differences between the hydrated sample and the dried, anhydrous form. How would the following errors affect the empirical formula for the compound? a. The student ran out of time and did not do the second heating. Explain how this error will affect the calculation for the number of moles of water in the hydrate? Will the final answer be artificially high or low? How do you know? b. The student recorded the mass of the cup + sample incorrectly and started with 2.2 g of hydrated compound but used 2.0 g in the calculations. Explain how this error will affect the calculation for the number of moles of water in the hydrate? Will the final answer be artificially high or low? How do you know?arrow_forwardPure hydrogen gas H2 Match the description below with the following microscopic pictures. More than one picture may fit the description.arrow_forward
- Part A) What principle states that the volumes of gases that combine in a chemical reaction are in the ratio of small whole numbers? A) Avogadro’s theory B) Law of constant conditions C) Law of conservation of volume D)Law of conservation of mass E) Law of combining volume Part B) Which of the following is not in the same ratio as the coefficients in a balanced chemical equation? A) Volumes of gaseous reactants and products B) Moles of reactants and products C) Molecules of reactants and products D) Masses of reactants and products E) None of the above Part C) What happens to the pressure of a gas if the number of molecules increases twofold (volume and temperature remains constant) A) The pressure decreases twofold B) The pressure remains constant C) The pressure decreases fourfold D) The pressure increases fourfold E) The pressure increases twofoldarrow_forwardThe great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. Suppose 48.0mL of dioxygen gas are produced by this reaction, at a temperature of 100.0°C and pressure of exactly 1atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.arrow_forwardHow do I solve this: 282.5g / 1mol (1 molecule / 1.189 x 10-21)= The "/" are supposed to be fraction strokes. It's supposed to be an Avogadro's number estimate. Where the mass of one oleic acid molecule (1.189 x 10-21) is used to determine the number of oleic acid molecules required to give a mass of 282.5garrow_forward
- A sample contains FeS2. At the end of its gravimetric determination, BaSO4 is weighed and the percentage of Fe is being searched for. What is an expression for the gravimetric factor in this determination? (The formulas represent the formula weights) a) FeS2 / BaSO4 b) Fe /2 BaSO4 c) 2 Fe / BaSO4 d) FeS2 / 2 BaSO4 e) 2 FeS2 / BaSO4arrow_forward1) When the sample is first put into the crucible and heated, the directions say to heat gently for the first five minutes. why do you suppose this is important? 2) Suppose that some of the compounds spilled out of the crucible after it was heated. Would that cause the percent by mass of water in the compound determined by the experiment to be too low, too high, or unchanged? Briefly explain your answer. 3) The unknown compounds used in this experiment are the following compounds. Based on your experimental results, what is the identity of the unknown compound you used? Show all calculations needed. Compound: CaSO4. 2H2O, MgSO4.7H2O, BaCl2.2H2O, ZnSO4.7H2Oarrow_forwardAspirin or acetyl salicylic acid is synthesized by reacting salicylic acid with acetic anhydride: C7H6O3 (salicylic acid) + C4H6O3 (acetic anhydride) = C9H8O4 (aspirin) + C2H4O2 (acetic acid) (a) How much salicylic acid is required to produce 0.400 g of aspirin (about the content in a tablet), assuming the acetic anhydride is present in excess? (b) Calculate the amount of salicylic acid needed if 74.9% of salicylic acid is converted to aspirin. (c) In one experiment, 9.26 g of salicylic acid is reacted with 8.54 g of acetic anhydride. Calculate the theoretical yield of aspirin and the percent yield if only 10.9 g of aspirin is produced.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning