Please send me the question in 30 minutes it's very urgent plz both questions 6 and 7 than rating helpful Question 6Determine the mass of iron (III) chloride that is needed to completely react with 596.1 mL of 96.89 mM sodium sulfide in a doubledisplacement reaction that produces solid Fe2S3. Report your answer in grams.Add your answerQuestion 7Determine concentration of sulfide (S2) the remains when 60.88 mL of 0.165 M iron (III) chloride is combined with 236.59 mL of 885mM sodium sulfide in a double displacement reaction that produces solid Fe2S3. Report your answer in mM.Add your answer

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Question 6 Determine the mass of iron (III) chloride that is needed to completely react with 596.1 mL of 96.89 mM sodium sulfide in a double displacement reaction that produces solid Fe₂S3. Report your answer in grams. Add your answer

Question 6 Determine the mass of iron (III) chloride that is needed to completely react with 596.1 mL of 96.89 mM sodium sulfide in a double displacement reaction that produces solid Fe₂S3. Report your answer in grams. Add your answer

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 134IP: On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado....

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hich of the following statements is true for the reaction of nitrogen gas with hydrogen gas to produce ammonia (NH3)? Choose the best answer. l type='a'> Subscripts can be changed to balance this equation, just as they can he changed to balance the charges when writing the formula for an ionic compound. i>The nitrogen and hydrogen will not react until you have added the correct mole ratios. i>The mole ratio of nitrogen to hydrogen in the balanced equation is 1:2. i>Ammonia will not form unless 1 mole of nitrogen and 3 moles of hydrogen have been added. i>The balanced equation allows you to predict how much ammonia you will make based on the amount of nitrogen and hydrogen present.
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
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