Answered: C. Reactivity of metals: 1.…

C. Reactivity of metals: 1. Observations (Indicate whether the reaction occurred, the vigor, extent and speed): Al Cu Zn b. а. Al (SO.)3 d. C. CuSO4 f. e. ZnSO4

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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omework 104 A CM/Team Time x Homework 103 x Hornework 102 structure.com/courses/943/assignments/16424 Homework 104 Due: Fri Mar 12, 2021 8:00am Unlimited Attempts Available 1. Given the following reaction, answer the questions that follow: C,H3 + 5 O2 → 3 CO, + 4 H,0 a) If you begin with 3.5 moles of C,H, and 6.2 moles of O,, find the moles of carbon dioxide produced. b) Find the mass of CO, produced using your work in step (a) above.
MN IN The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in the stratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCS) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine was previously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone. (1) CIO(g) + O,(g) → Cl(g) + 20,(g) AHxn = -122.8 kJ AHn = -285.3 kJ | rxn AHn = ? (3)°O + (3)OIƆ (3)1Ɔ+(3)*o (£) (3) 0E – (3)°07 (2) rxn %3D = UXHV kJ MacBook Pro Q Search or enter website name The & %23 $4 3. 4. 5. 7. 6. delete R H. K. re B. HE MOSISO command option
At 40^0c, H202 (aq) will decompose according to the foll. reaction: 2 H202 (aq) ----2H20(l) +02 (g) The foll. data were collected for the concentration of h202 at various times. Time. [H202] (mol/L) 0. 1.600 3.10*10^4 0.592 6.20*10^4. 0.219 (a) Calculate the average rate of decomposition in H202 between0 and 3.10 * 10^4 s. use this rate to calculate the average rate of production 02 (g) over the same time period. (b) What are these rates for the time period 3.10*10^4 s. to 6.20 *10^4 s.? Rate of H202 decomposition Rate of O2 Production
ab and Mastering 7 > 2 F2 W S You may want to reference (Pages 245-246) Section 7.8 while completing this problem. # Calcium cyanamide reacts with water to form calcium carbonate and ammonia via the following reaction: CaCN₂ (s) + 3H₂O(1)→ CaCO3(s) + 2NH3(g) 3 E O 80 F3 D h My Questions | bartleby $ 4 2008 F4 R F % 5 F5 T openvellum.ecollege.com G ^ 6 How many grams of water are needed to react with 71.0 g CaCN₂? 195] ΑΣΦ 5 → mass H₂O = F6 Submit Part B Y How many grams of NH3 are produced from 5.22 g CaCN₂? 4 IVE ΑΣΦ mass NH3 = Submit Part C Request Answer mass CaCO3 = MacBook Air Request Answer H E Course Home How many grams of CaCO3 form if 156 g water react? Copyright © 2022 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us | & 7 44 F7 U IVE ΑΣΦ 5 Pearson *00 8 J DII F8 I 1 C → C ( 9 K Ċ DD F9 0 ? -0 ? ? L g g P 7.8: Mass Calculations for Chemical Reactions Review | Constants I Periodic Table g F10 P : (1 F11 { + 11 Ⓒ+ [ 11 1 F12…
In the reaction being studied in this lab, solutions of hydrogen peroxide, H2O2, and potassium permanganate, KMnO4, will be combined in acidic solution. KMnO4, will be used as the titrant to analyze the concentration of hydrogen peroxide in a drugstore bottle. The KMnO4 solution is purple in color, as it is added to the hydrogen peroxide solution, it reacts with the H2O2 to produce colorless Mn2+, and thus the color will fade in the flask. When all the H2O2has been used up, the last drop of potassium permanganate that is added will keep its color. The endpoint of the titration is the point at which the last drop of KMnO4 added to the solution causes it to turn pink. The balanced equation for the reaction in this lab is: 2MnO4‒(aq) + 5H2O2(aq) + 6H+(aq) à 2Mn2+(aq) + 5O2(g) + 8H2O(l) 1. What is the titrant in this lab? 2. What is the analyte in this lab? 3. The balanced equation for the reaction in this lab is: 2MnO4‒(aq) + 5H2O2(aq) + 6H+(aq) à 2Mn2+(aq) + 5O2(g) + 8H2O(l)…
Consider the following reaction: The following is a plot of the conc a startíng point of 1.0 M A2 and 1. AB (blue) over time. 30.75
Identify the oxidizing agent in the chemical reaction 5Fe+2(aq) + MnO4-(aq) + 8H+(aq) 5Fe+3 + Mn+2(aq) + 4H2O(l) The answer is ……………………………… Calculate the total number of atoms in 500 Ml OF 0.200 M KNO3 solution. The answer is ……………………………… Mg has three stable isotopes. Given a sample of Mg with the following masses and percent abundances: 24Mg: 23.9850 amu, 58.42% 25Mg: 24.9858 amu, 15.22% 26Mg: 25.9826 amu, 26.36% The average atomic mass (in amu) is …………………… What mass of Na2SO4 is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125 M The answer is ………………………
20. The Haber-Bosch process, devised in the early 20th century, revolutionized global industry. It provides a way of“fixing” atmospheric nitrogen into ammonia, allowing for the production of fertilizers and the many nitrogenbased chemicals we use today. The reaction is carried out in numerous industrial facilities all over the world:
Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposes spontaneously but slowly. The decomposition reaction will proceed at a faster rate if iodide ion, a catalyst, is added. The steps for the catalyzed reaction are: H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq) OO H₂O₂(aq) + Ol(aq) → H₂O(l) + O₂(g) +1-(aq) a. What is the net reaction? b. If 10.00 mL of H₂O₂ undergoes this reaction, what mass of oxygen is produced? c. If the reaction has an 85.5% yield, what mass of oxygen is actually produced?
C. DECOMPOSITION REACTION : AB >A + B 1. _KCIO3 > KCI + _O2 2. Hg + _O2 H2CO3 → H2O + _CO2 NH4NO3 > H2O + N2O NANO3 > NaNO2 + O2 (g) 3. 4. 5.
Thiosulfate ions are oxidized by iodine according to the reaction below:2 S2O 33- (aq) + I2 (aq) → S 4O 62- (aq) + 2I -(aq)If 0.0080 mol of S2 O32- is consumed in 1.0 L of solution every second, what isconsumption rate of iodine?
QUESTION 5 2H2O(1) 2H2(g) a. Combination b. Decomposition c. Single Replacement O d. Double Replacement + O2(g) QUESTION 6 CaCl2(s) Ca(s) + Cl2(g) a. Combination b. Decomposition c. Single Replacement O d. Double Replacement