T-Mobile 12:19 PM 66% Question 45 of 59 Submit Determine the number of molecules of Cr2O3 that form when 1.34 x 103 g of oxygen completely reacts according to the following equation: 4 Cr(s) + 3 O2(g) → Cr2O3(s) х STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 1.34 x 103 4.24 x 103 g Cr 52.00 2.52 x 1025 mol Cr mol 3 32.00 3.78 × 1025 g O2 4 152.00 mol O2 6.022 x 1023 1.68 x 1025 g Cr2O3

T-Mobile 12:19 PM 66% Question 45 of 59 Submit Determine the number of molecules of Cr2O3 that form when 1.34 x 103 g of oxygen completely reacts according to the following equation: 4 Cr(s) + 3 O2(g) → Cr2O3(s) х STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 1.34 x 103 4.24 x 103 g Cr 52.00 2.52 x 1025 mol Cr mol 3 32.00 3.78 × 1025 g O2 4 152.00 mol O2 6.022 x 1023 1.68 x 1025 g Cr2O3

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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Could I have help with these two questions homework questions im not really understanding this unit
In the following reaction, oxygen is the excess reactant.SiCl4 + O2 → SiO2 + Cl2The table shows an experimental record for the above reaction. Experimental Record Trial Starting Amount of SiCl4 Starting Amount of O2 Actual Yield of SiO2 1 120 g 240 g 38.2 g 2 75 g 50 g 25.2 g Calculate the percentage yield for SiO2 for Trial 1. Also, determine the leftover reactant for the trial. Show your work. Based on the percentage yield in Trial 2, explain what ratio of reactants is more efficient for the given reaction.
Chemistry part c is incorrect the answer is not 0.
Question 6 of 8 Submit Determine the number of grams of CaH10 that are required to completely react to produce 8.70 mol of CO2 according to the following combustion reaction: 2 C.H10(g) + 13 O:(g) 8 CO:(g) + 10 H:O(g) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 2 8.70 6.022 x 1023 2.18 0.0374 44.01 4.35 208.00 13 18.02 126 10 58.14 1 g O. g H2O g CO2 mol CO2 mol O2 mol CAH10 mol H2O g CH10
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Dilution Problems, Chemistry, Molarity & Concentration Examples,... M O O CHEMICAL REACTIONS Reaction sequence stoichiometry In the second step, iron(III) oxide and carbon monoxide react to form iron and carbon dioxide: Fe₂O3(s) + 3CO(g) → 2Fe(s) + 3 CO₂ (g) E crosoft O V Blast furnaces extra pure iron from the iron (III) oxide in iron ore in a two step sequence. In the first step, carbon and oxygen react to form carbon monoxide: 2C(s) + O₂(g) 2 CO (g) W Suppose the yield of the first step is 84.% and the yield of the second step is 63.%. Calculate the mass of oxygen required to make 3.0 kg of iron. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. G Microsoft Microsoft 6.52.210... Explanation BO C Check 9,269 x10 믐 103 X OCT 24 ロ・ロ átv 2 3/5 DOZA Simrat 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility W E ol Ar
A 4.86 g quantity of solid rubidiummetal is combined with 3.44 g of magnesium chloride crystals according to this chemical reaction: 2 Rb (s) + 1 MgCl2 (s) 1Mg (s) +2 RbCI (s) What quantity of magnesium metal will be produced? _g Mg round your answer using appropriate sig figs The following molar masses may or may not be needed, but are provided to save you time: • molar mass: Rb = 85.47 g/mol • molar mass: MgCl2= 95.21 g/mol • molar mass: Mg = 24.31 g/mol Hiint: Start with the number of grams of Rubidium
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esc Calculate the quantity of O, would be required to generate 13.0 mol of NO in the reaction below assuming the reaction has only 72.4% yield. 2 NO (g) + O₂(g) → 2 NO₂ (g) ! 1 S Q A O @ 2 W S CE #3 E D $ 4 R % 5 F LL T MacBook Pro ^ 6 G Y & 7 FEB 21 H zoom U 8 W -
K $ 4 R For the following reaction, 4.16 grams of hydrogen gas are allowed to react with 45.2 grams of iodine hydrogen (g) + iodine (s)→ hydrogen iodide (g) What is the maximum amount of hydrogen iodide that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? Submit Answer % 5 [Review Topics] [References] Use the References to access important values if needed for this question. Show Hint T Retry Entire Group 4 more group attempts remaining Cengage Learning Cengage Technical Support < 6 Y d 7 U 8 I < ( 9 0 O P grams grams * Previous 4) [
Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O2 (g) → 2M9O (s) When 4.00 g of magnesium burms, the theoretical yield of magnesium oxide is g. A) 4.00 B) 6.63 C) 0.165 D) 3.32 E) 13.3 A D
Can someone answer this is the exact same way is supposed to on the site