[References]Use the References to access important values if needed for this question.For the following reaction, 0.466 moles of hydrochloric acid are mixed with 0.205 moles of iron(III) oxide.hydrochloric acid(aq) +iron(III) oxide(s)water(e) + iron(II) chloride(aq)What is the formula for the limiting reagent?What is the maxımum amount of water that can be produced?molesSubmit AnswerRetry Entire Group9 more group attempts remainingPreviousNext

The reaction taking place is 6 HCl (aq) + Fe2O3 (s) ------> 3 H2O (l) + 2 FeCl3 (aq) So from…

Answered: [References] Use the References to…

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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4.106. Aspirin (acetlsalicyclic acid) may be formed from salicyclic acid and acetic acid as follows:C7H6O3 (aq) + CH3COOH (aq) → C9H8O4(s) + H2O(l)Salicyclic acid Acetic Acid Aspirin b. How many mol of aspirin may be produced from 1.00*102 mol mol salicylic acid? c. How many g of aspirin may be produced from 1.00*102 mol salicylic acid? d. How many g of acetic acid would be required to completely with the 1.00*102 mol salicylic acid? e. For the conditions in part (d), how many g of aspirin would form?
3. A student mixes 100.0 mL of a 0.100 M solution of potassium phosphate with 100.0 mL of a 0.125 M solution of copper (II) sulfate and obtains a blue solid. (a) Write the balanced chemical equation for the reaction including physical states. (b) Determine the limiting reagent. (c) Calculate the number of moles of the excess reagent after the reaction is completed. Record servation
Use the References to access important values if needed for this question. Enter the coefficients directly from the balanced chemical equation. Do not reduce to lowest terms. For example: If 3 moles H, react with 3 moles 0,, enter "3" for each, not "1". According to the following reaction: 3Cl, (g) + 3H20 (1) → 5HCI (aq) + HClo3 (aq) What would you multiply "moles of chlorine" by to convert to the units "moles of chloric acid (HCIO3)" ? (number) (unit) moles Cl2 = moles HCIO3 (number) (unit)
Suppose we react 4.00 mol of HCl with 1.00 mol of Ca,(PO,), to produce phosphoric acid, H,PO, 4 according to the balanced reaction, 6 HCl(aq) + Ca,(PO,),(s) → 2 H,PO,(aq) + 3 CaCl,(aq) What reactant remains when the other is fully consumed, and how many moles of this reactant remain? A 0.33 mol of Ca,(PO,)2 B 0.66 mol of Ca,(PO,), C 1.00 mol of HCl i D 3.00 mol of HCl
Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4 HCI(aq) + MnO,(s) → MnCl, (aq) +2 H,O(1) + Cl, (g) A sample of 35.5 g MnO, is added to a solution containing 50.9 g HCI. What is the limiting reactant? HCI O MnO, What is the theoretical yield of CI,? theoretical yield: g Cl, If the yield of the reaction is 86.3%, what is the actual yield of chlorine? actual yield: g Cl,
How many moles of Agl will be formed when 75.0 mL of 0.300 M AGNO: is completely reacted according to the balanced chemical reaction: 2 AGNO:(aq) + Cal:(aq) – 2 Agl(s) + Ca(NO:):(aq) STARTING AMOUNT *( ) 6.022 x 1028 0.0450 0.300 75.0 1 234.77 0.250 1000 169.88 22.5 0.001 0.0225 2 mL Agl mol AGNO: g Agl mol Agl mL AGNO: g AGNO: MAGNO. LAgl LAGNO:
a) Indicate the reaction type that is taking place in the reactions below: b) Write the balanced molecular equation and the (c) Net lonic equation for the reactions below: (1) When aqueous solutions of strontium nitrate and potassium phosphate are mixed: (2) When aqueous solutions of H₂CO3 and LIOH are mixed: (3) When K3PO4(aq) + Sr(NO3)₂(aq) are mixed:
3.4 A 5.17 g sample of vinegar is titrated with 0.018 M NaOH. If the vinegar requires 42.3 mL of the NaOH solution for complete reaction, what is the mass percentage of acetic acid in the vinegar? (i.e. calculate the % of CH3COOH in the vinegar) The reaction is: NaOH(aq) + CH3COOH(aq) H2O(l) + NaCH3COO (aq) M,(CH3COOH) = 60.0
If a solution containing 58 g of mercury(II) nitrate is allowed to react completely with a solution containing 16.642 g of sodium sulfate according to the equation below: Hg(NO3)2(aq)+Na2SO4(aq)------2NaNO3(aq)+HgSO4(s) A. How many grams of solid precipitate will be formed if the reaction has a 100% yield? B. How many grams of the excess reagent will remain after the reaction? C. If the reaction has only an 80% yield, how many grams of solid precipitate will be formed?
Many compounds are only partially dissociated into ions in aqueous solution. Trichloroacetic acid (CC13 CO₂H), for instance, is partially dissociated in water according to the equation CC13 CO₂ H(aq) → H+ (aq) + CC13 CO₂ (aq) For a solution prepared by dissolving 1.00 mol of trichloroacetic acid in 1.00 kg of water, 37.0 % of the trichloroacetic acid dissociates to form H+ and CC13 CO₂ ions. What is the total concentration of dissolved ions and molecules in 1 kg of water? Express your answer using three significant figures. VE ΑΣΦ Submit Request Answer ? mol/kg
Consider the following reaction: (reaction in image), what mass of AI2(SO4)3 will be produced from 355 mL of 0.200 M H2SO4 solution? ___ g (provide answer to correct sig figs in units of g)
Balance each of the following equations that describe decomposition reactions. SaSO4(s)=CaO+SO3(g) ‍‍Li2CO3(s)=Li2O(s)+CO2(g) L‍‍iHCO3(s)=Li2CO3(s)+H2O(g)+CO2(g) C‍6H6(l)=C(s)+H2(s) PBr3(l)= P4(s)+Br2(l)

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