11.T/ Write a balanced chemical equation for eachchemical reaction.a. Solid potassium reacts with gaseous chlorine toform solid potassium chloride.c. Nitrogen gas and hydrogen gas react to formgaseous ammonia.12. TI Barium hydroxide can react with phosphoricacid to form barium hydrogen phosphate and water:Ba(OH)2(s) + H;PO,(aq) → BaHPO4(s) + H,O(t)c. Write the balanced chemical equation.

Answer Write the balance chemical equation

Answered: 11. T Write a balanced chemical…

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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3. Zinc reacts with acids according to the following equation; Zn(s) + 2HA(aq) → Zn(A),(aq) + H,(g) The net ionic reaction is; Zn(s) + 2H,O*(aq) → Zn2*(aq) + H,(g) Hydrochloric acid is a strong acid and acetic acid is a weak acid. Based on the above information, explain the difference in the two reaction rates.
Fe"(aq) + OH (aq) 2. Metals in Water Write the products (except for letter d) and balance the chemical equation. Write NR on the products side if there is no reaction. a. Mg(s) + H201) → b. Zn(s) + H2O() → C. Cu(s) + H20(1) → d. Fe(s) + H2O(g) → FeO(s) + H2(9) Fe2* (aq) + OH(aq) + e- → Fe(OH)3(aq)
Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent. redox reaction? O yes O no 30, (g) + 4Fe(s) 2Fe,0, (s) reducing agent: ? oxidizing agent: redox reaction? O yes O no CaO(s) + CO,(g) CaCO,(s) reducing agent: oxidizing agent: redox reaction? O yes O no 70, (g) + 2CH, CH, (8) → 4CO,(g) + 6H,0(g) reducing agent: oxidizing agent:
8. Sodium thiosulfate, Na2S₂O3, is an important reagent for titrations. Its solutions can be standardized by titrating the iodine released when a weighed amount of potassium hydrogen iodate, KH(IO3)2 (389.912 g/mol), is allowed to react with excess potassium iodide in acidic solutions. The net ionic equations are: production of iodine from KH(IO3)2: IO3¯¯ +5 I¯¯+ 6H* → 3 1₂ + 3 H₂O 1₂+2 S₂03² → 2 I¯+S406²- 2- titration of iodine: What is the molarity of a sodium thiosulfate solution if 39.66 mL are required to titrate the iodine released from 0.1022 g of KH(IO3)2?
1801 2. If the density of a 2.50 M HCl solution is 1.248 g/cm3, what mass of HCL solution is needed to react with 82.07 mL of 1.54 M Mg(OH)2? The chemical reaction is: HCI + Mg(OH), → MgCl, + H,O
65. Balance each of the following equations that describe decomposition reactions. a. CaSO4(s) CaO(s) + SO3 (g) b. Li, CO3 (s) → Li, O(s) + CO2 (9) c. LIHCO3 (s) → Li, CO3 (8) + H2 O(9) + CO2(g) d. C6 H6 (1) → C(s) + H2 (g) e. PB13 (1) → P4(s) + Br2 (1)
When aqueous solutions of iron(II) bromide and sodium carbonate are combined, solid iron(II) carbonate and a solution of sodium bromide are formed. The net ionic equation for this reaction is: When aqueous solutions of potassium nitrite and hydroiodic acid are mixed, an aqueous solution of potassium iodide and nitrous acid results. Write the net ionic equation for the reaction. When solid Zn metal is put into an aqueous solution of Sn(NO3)2, solid Sn metal and a solution of Zn(NO3)2 result. Write the net ionic equation for the reaction.
b. 3H2SO4(aq) + 2Al(OH);(aq) → Al2(SO4)3(aq) + 6H2O(1) 4. In each of the following, identify the reactant that is oxidized and the reactant that is red a. 2Li(s) + F2(g) → 2LİF(s) b. Cl2(g) + 2KI(aq) → I2(s) + 2KCI(aq) atoms of H 5. Calculate each of the following a. number of Li atoms in 4.5 moles ofLi. b. moles of Cu in 7.8 x 10²1 atoms of Cu. c. moles of C2H6 in 3.75 x 1023 molecules of C2H6.
65. Lead ions can be precipitated from solution with NaCl according to the reaction: Pb²+ (aq) + 2 NaCl(aq) PbCl₂(s) + 2 Na+ (aq) When 135.8 g of NaCl are added to a solution containing 195.7 g of Pb²+, a PbCl2 precipitate forms. The precipitate is filtered and dried and found to have a mass of 252.4 g. Determine the limiting reactant, theoretical yield of PbCl2, and percent yield for the reaction.
Classify each chemical reaction: Ba (CIO,),(s) → BaCl,(s) + 30, (8) KOH(aq) + HBrO (aq) 1 reaction CuSO4 (aq) + Zn CrO4 (aq) K BrO (aq) + H₂O (1) CH₂OCH₂ (1) + 30₂(g) → 2CO₂(g) + 3H₂O(g) ZnSO4 (aq) + Cu Cro(s) type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition 000 000 000 precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base
* CO (be • Part C Na + HCI→ Express your answer as a balanced equation including states of matter. Write "NR" if no reaction occurs. P3V 2Na(s) + 2HC1(g)→2NaCl(aq) + H, (g) Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Part D Na + Ca2+ Express your answer as a balanced equation. Do not include states of matter. Write "N.R." if no reaction occurs. DA chemical reaction does not occur for this question. Submit Request Answer Provide Feedback P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy Permi G Search or type URL %23 %$4 i 4. 5. 3. F.
15. If 23.0 mL of a 1.00 M Ba(NO3)2 solution was reacted with 55.0 mL of a 0.700 M solution of K3PO4 to produce the solid Ba3(PO4)2 by the balanced chemical equation 3 Ba(NO3)2 (aq) + 2 K3PO4(aq) – Ba3(PO4)2(s) + 6 KNO3(aq) a. What is the limiting reagent? AS b. How many grams of Ba3(PO4)2 will be produced? elomibt.ESE -3HA

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