Using "-->" as your reaction arrow and the correct subscript and superscripts as needed, please balance the following reaction under basic conditions:I⁻ + MnO₄⁻ --> I₂ + MnO₂For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac).---There are no graphs or diagrams in this image. The image shows a section of a text editor interface, including a toolbar with various formatting options. The toolbar includes icons for formatting text (bold, italic, underline), paragraph styles, font choices (Arial, 10pt), alignment options, bullet points, tables, superscripts and subscripts, and other formatting tools.

Answered: Image /qna-images/answer/8e2f092f-74d0-4eb5-8034-78f46616054f.jpg

Using "-->" as your reaction arrow and the correct subscript and superscripts as needed, please balance the following reaction under basic conditions: I-+ MnO4 → 12+ MnO2 For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). BIUS Paragraph V Arial ABC V ✓ ¶T "Ω Θ 10pt 田租用网 AV 图图 Ť () Ix 26 10

Using "-->" as your reaction arrow and the correct subscript and superscripts as needed, please balance the following reaction under basic conditions: I-+ MnO4 → 12+ MnO2 For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). BIUS Paragraph V Arial ABC V ✓ ¶T "Ω Θ 10pt 田租用网 AV 图图 Ť () Ix 26 10

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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The reduction of iron(III) oxide to iron during steel-making can be summarized by this sequence of reactions: 20(s) +0, (g) =2 CO (g) K, Fe,0, (s) +3 CO (g) =2 Fe (1) +3 CO, (g) K2 The net reaction is: 2 Fe,O, (s) +6C (s) +30, (g)=4 Fe (1) +6CO, (3) K Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K, and K,. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator. K = 믐 Submit Assign Continue MacBook Air F7 000 吕口 000 FA F5
The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3 and water: 2Al(OH)3(s) + Al2O3(s) -> 3H2O(g) In the second step, alumina Al2O3 and carbon react to form aluminum and carbon dioxide: 2Al2O3(s) + 3C(s) + 4Al(s) -> 3CO2(g) Suppose the yield of the first step is 74.% and the yield of the second step is 76.% . Calculate the mass of aluminum hydroxide required to make 4.0kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
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.
Hexamethylenediamine (C6H16N2) is one of the starting materials for the production of nylon. It can be prepared from adipic acid (C6H1004) by the following overall reaction: C6H1004(/) + 2 NH3(g) + 4 H2(g) → C6H16N2(/) + 4 H20(/) Click here to see the production of nylon. What is the percent yield if 217.2 g hexamethylenediamine is made from 433.6 g adipic acid? %
Drag and drop the appropriate choices to fill in the following chemical reaction: where you start the reaction with 2 moles of C2H60 and 3 moles of 02. The Limiting Reactant is O2 Reaction Table C2H60 3 2 H20 CO2 (g) + (g) (g) + 02 (g) Initial Change Final 0123 || 4 +1 -1 +2 -2 | +3 -3 |+4-4 +5 -5
← ALEKS-Alasia aqua C с www-awu.aleks.com = gro-Islere to u toNsikr7 8P3 H-1BjuJnuCDtT6kRBabGFF3MOAKZ_UVXON202geoxT1611PLTg4B/XE3ZhcVVdG_Sanal98wrHEROCK O CHEMICAL REACTIONS Identifying the limiting reactant in a drawing of a mixture The drawing below shows a mixture of molecules: carbon Explanation key Ooxygen O hydrogen nitrogen O Check sulfur Suppose the following chemical reaction can take place in this mixture: 2 C₂H₂(g) +50₂(g) → 4 CO₂(g) + 2 H₂O(g) chlorine Of which reactant are there the most initial moles? Enter its chemical formula: Of which reactant are there the least initial moles? Enter its chemical formula: Which reactant is the limiting reactant? Enter its chemical formula: 800 X Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use
Mg + 2HCl → MgCl2 + H2 This experiment was performed two times. All values are valid to one decimal place. If the decimal place is not shown, add a ".0" Experiment Mass of Mg (mg) Starting Temperature (°C) Final Temperature (°C) 1 2 19.6 20.7 19.5 20.7 33 33.5 The previous page contained data from two experimental runs for the reaction between magnesium and hydrochloric acid. Mg+ 2HC! MgCl2 + H2 First, how many moles (n) of Mg reacted with the HCI? Use the average value of the two masses from your provided data set. Answer: 0.001658 I Mg + 2HCI MgCl2 + H2 Next, what is the amount of heat absorbed by the water (qsurr) in the experiment? Use the average AT from your data to calculate a single value for q. Report your answer in J. Remember to consult the lab manual and/or the video for any values you might need. Answer: Mg + 2HC! MgCl2 + H2 Finally, calculate A,H for this reaction and report your answer in kJ/mol. Answer:
ll Boost LTE 2:01 AM O 60% Question 6 of 6 Submit Determine the number of grams of C4H10 that are required to completely react to produce 8.70 mol of CO2 according to the following combustion reaction: C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H20(g) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) X 6.022 x 1023 4.35 13 0.0374 18. 8.70 126 208.00 8 2. 10 58.14 44.01 Tap here or pull up for additional resources 2.
M Your Chemistry answe × b Answered: Balance th x ← с app.101edu.co < + D2L Quiz Submissions - Chapter 12 X Aktiv Chemistry + Write a balanced chemical equation based on the following description: solid ammonium carbonate decomposes into ammonia gas, carbon dioxide gas and water vapor. (NH,),CO,(s) 1 ₁ + ■ Reset X b Success Confirmation X | G "The flickering light of × + O U 2 3 □2 ☐ 3 OC ) 4 Time's Up! CO LO 5 05 + C 0²+ 6 7 8 07 = (s) N 3+ (1) D2L Quiz 10-12 - Spring 20 X b Success Confirmation x + • x H₂O 4+ 9 0 ☐9 口。 (g) (aq) H Delete Update: Submit
riment 3. Chemicals in Everyday Life: What are they and how do we know? - Post-lab %3D -iment 3- Post-Lab - Manual Question 3 - Copy %3D %3D Part A Write the overall reaction between aqueous HCl and solid Na2 CO3 to form sodium chloride, water, and carbon dioxide. Write a balanced reaction including states of matter ΑΣφ ? A chemical reaction does not occur for this question. Submit Request Answer Part B nodium chloride, water, and carbon dioxide.
Be sure to answer all parts. Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: Hint oints Solution 5Ca + V,05- 5CAO + 2V eBook Guided Solution Print In one process, 1.540 x 10° g of V,O5 react with 2.120 × 10³ g Ca. References (a) Calculate the theoretical yield of V. (b) Calculate the percent yield if 815.0 g of V are obtained. Report your answers to the correct number of significant figures. Next > Mc Graw Hill Prev 4 of 45 31°C Mostly sunny P Type here to search 1080 Jade Pa F12 Prt Sc F11 F10 NumLk F8 F9 F7 F6 E5
(3) A container holding NO2 and CO gas will lose NO2 gas via the reaction NO2 (g) + CO (g) → NO (g) + CO2 (g) A chemist measures the [NO2] over time and finds that plotting 1/[NO2 ] versus time yields a straight line with a slope of 3.56×10-2 M-1·s-1. If the container originally held 1.00 M NO2, what is the concentration of NO2 after 1.50 hour [NO2]1.5 hrs = ___________ How long will it take the [NO2] to drop to 20% of its initial concentration of 1.00 M? T20% = __________