b2 Empirical Formula MG Su21 (7) - Protected View - Saved to this PC -MailingsReviewViewHelpLayoutReferencesEnable Editinget can contain viruses. Unless you need to edit, it's safer to stay in Protected View3. What physical property of water and HCl allows us to separate them from thezinc-chlorine compound produced in the reaction? How?4.Name:Empirical Formula Lab4. Imagine that during the experiment, a group allows their sample to get too hotso that some sample of the zinc-chlorine compound spatters out of the dish.When they calculate the percent by mass of zine in the compound, will thecalculated percent be higher or lower. Really think it through Explain144fho%&4.78.9.

Solution: We know the solubility principle i.e. likes dissolves like. Since HCl is the strong acid…

3. What physical property of water and HCl allows us to separate them from the zinc chlorine compound produced in the reaction? How? Name: Empirical Formula La 4. Imagine that during the experiment, a group allows their sample to get too hot so that some sample of the zinc-chlorine compound spatters out of the dish. When they calculate the percent by mass of zinc in the compound, will the calculated percent be higher or lower. Really think it through Explain

3. What physical property of water and HCl allows us to separate them from the zinc chlorine compound produced in the reaction? How? Name: Empirical Formula La 4. Imagine that during the experiment, a group allows their sample to get too hot so that some sample of the zinc-chlorine compound spatters out of the dish. When they calculate the percent by mass of zinc in the compound, will the calculated percent be higher or lower. Really think it through Explain

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...

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13. A chemistry student offers a possible improvement to this lab. Since one goal of this lab is to determine the mass of the precipitate produced, wouldn't it be possible to measure the mass of an empty beaker, mix the solutions, and boil off the water until it is entirely evaporated, leaving only solid behind? Then the beaker with the precipitate could be weighed, and the difference between this mass and that of the empty beaker would be the mass of the precipitate. This would eliminate the need for the filtration step. Explain why this is a poor suggestion. Remember to check your reasoning on this question and all other questions with your instructor.
Name Lab Partner Section # Date Pre-Lab Assignment: Stoichiometry Lab 1. In a lab experiment similar to the one you are going to do, a student slowly added hy- drochloric acid (HCI) to an evaporating dish containing magnesium carbonate MgCO3. a. Complete and balance the following equation for the reaction between magnesium carbonate and hydrochloric acid. MgCO3 (s) + HCl (aq) → (aq) + H₂CO3(aq) (When writing the formula for the missing product did you consider the charges of the ions?) b. When carbonic acid is formed in a chemical reaction, it is unstable and immedi- ately decomposes into carbon dioxide and water. Rewrite the equation above to show the final products using this information.
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w CHAPTER 4-STOICHIOMETRY: QUANTITATIVE INFORMATION ABOU → Previous Page Page 5 5 of 9 of 9 Next > If you dilute 35.0 mL of 2.25 M hydrochloric acid to 550. mL, what is the molar concentration of the dilute acid? OCT 12 Molar concentration = 2 2 tv # 3 M NIEZA $ W Document3.docx 115 54 FANTASAAYOerene % 5 181WP Conver MacBook Pro 6 NA Oct 10. 2022 at E Awe
How can we answer these questions on solution stoichiometry and equilibrium?
a. A 2.0 M potassium chloride solution is prepared by dissolving 37.3 g of potassium chloride in distilled water. What is the volume of the solution formed?(Relative atomic masses: K = 39.1, Cl = 35.5) b. What volume of 0.05 M Na2CO3 solution can be prepared from 2.65 g of Na2CO3?(relative atomic mass Na=23.0, C=12.0, O=16.0) c. Which of the following apparatus is usually used to deliver 25.0 cm3 of a solution into a conical flask?A. BuretteB. PipetteC. Beaker D. Volumetric flask
Suppose the following chemical reaction can take place in this mixture
18-please fast The Hall process for the production of aluminum involves the reaction of aluminum oxide with elemental carbon to give aluminum metal and carbon monoxide. If the yield of this reaction is 82% and aluminum ore is 71% by mass aluminum oxide, what mass of aluminum ore must be mined in order to produce 1.0 × 103 kg (1 metric ton) of aluminum metal by the Hall process? Select one: a. 1.6 × 103 kg b. 2.2 × 103 kg c. 1.8 × 103 kg d. 1.1 × 103 kg e. 3.3 × 103 kg
Consider the following chemical reactions: KClO3 (s) ----------> KCl(s) + O2(g) NaNO3(s) ---------> NaNO2(s) + O2(g) 5.0000 g mixture of potassium chlorate and sodium nitrate is decomposed and the mass of residuals is 3.8600 g. The oxygen gas is collected in 359. mL. container at 25 oC by water displacement technique. Calculate the total pressure in mmHg. the vapor pressure of H2O at 25oC is 18.3 mmHg. K = 39.10 g/mole, Cl = 35.45 g/mole, Na = 22.99 g/mole, N = 14.00 g/mole and O = 16.00 g/mole
Please help with question 2 G-I
An unknown hydrated compound (AC·XH2O) contains 35.9% H2O. The molar mass of the anhydrous compound (AC) is 159.61 g/mol. Find the water of crystallization in this unknown hydrate. Part B is to find the number of moles of anhydrous compound (AC).
. Table 1. Volumes of NaOH solution needed to titrate 25.00mL of HCI Concentration Initial of NaOH(M) Final Volume Unknown volume Volume(mL) | (mL) of concentration (mL) NaOH (M) of HCI Trial 1 0.0963M 26.4 25.4 Trial 2 0.0963M 0.3 25.4 25.1 Trial 3 0.0963M 0.1 24.8 24.7 Average concertation of HCI (M)