a. Classify the type of reaction (double replacement, decomposition, combustion, etc)b. Predict the products if necessaryc. Balance the equationd. Write the net ionic equation for reactions involving aqueous solutions. Don't forget phase labels andcharges on ions. If no reaction write NR under the equation.Type of ReactionCH1,OH(1) + O2(g) →(NH.);PO(ag) + FesO ag) >la) Draw the Lewis Dot diagrams that obey the octet rule for the following covalent molecules. Then useVSEPR to determine the molecular shape of each molecule.1. NH32.SO2 1) a) Sulfuric acid, the industrial chemical produced in the greatest quantity each year, is prepared bythe reaction of sulfur in the presence of oxygen and water as described in the balanced chemicalequation below. Calculate the volume, in ml, of 18.0 M sulfuric acid solution that can be prepared fromthe reaction of 1850 g of sulfur with 6.50x10ʻmL oxygen gas at 25°C and 0.965atm and plenty of water.25(solid) + 30: (gas) + 2H20(liquid) > 2H;SO4(aqueous)b. Which substance is the limiting reactant? Explain how you know.

Answered: Image /qna-images/answer/3d6c8c19-262b-4b3f-8683-4a7283c00d72.jpg

a. Classify the type of reaction (double replacement, decomposition, combustion, etc) b. Predict the products if necessary c. Balance the equation d. Write the net ionic equation for reactions involving aqueous solutions. Don't forget phase labels and charges on ions. If no reaction write NR under the equation. Type of Reaction CH1,OH(1) + O2(g) → (NH.);PO(ag) + FesO ag) > la) Draw the Lewis Dot diagrams that obey the octet rule for the following covalent molecules. Then use VSEPR to determine the molecular shape of each molecule. 1. NH3 2.SO2

a. Classify the type of reaction (double replacement, decomposition, combustion, etc) b. Predict the products if necessary c. Balance the equation d. Write the net ionic equation for reactions involving aqueous solutions. Don't forget phase labels and charges on ions. If no reaction write NR under the equation. Type of Reaction CH1,OH(1) + O2(g) → (NH.);PO(ag) + FesO ag) > la) Draw the Lewis Dot diagrams that obey the octet rule for the following covalent molecules. Then use VSEPR to determine the molecular shape of each molecule. 1. NH3 2.SO2

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...

See similar textbooks

Similar questions

2. A double replacement reaction occurs between sodium hydroxide and copper(II)nitrate. a. Write the balanced equation for this reaction. (Note: Be sure to include the states of all reactants and products). b. Write the complete ionic equation for this reaction. (Note: Be sure to highlight the spectator ions in this reaction.) c. Write the net ionic equation for this reaction.
What is the net ionic equation for any precipitation reaction that may occur when solutions of NaOH and Cu(NO3)2 are mixed. a. No precipitation reaction will occur b. Na+(aq) + NO3-(aq) → NaNO3(s) c. Cu2+(aq) + 2 OH-(aq) → Cu(OH)2(s) d. Cu+(aq) + 2 NO3- → Cu(NO3)2(s)
Two solutions are mixed, and the resulting reaction produces NaNO3(aq) and NiCO3(s). a. Write the balanced molecular equation for this reaction. b. Write the net ionic equation, given that the sodium and nitrate ions are the spectator ions.
The chemical equation below, FeCl3(aq) + 3NaOH(aq) → Fe(OH)3(s) + 3 NaCl(aq) is an example of what type of reaction? A.) acid-base B.) combustion C.) oxidation-reduction D.) precipitation
1. Write balanced total ionic equations for the following double displacement reactions. Indicate the state of all reactants and products (eg. (aq) for aqueous, (s) for solid). (See pages 45-47 and 54 in the lab manual for more information) a. Pb(NO3)2 + HCI b. Fe(NO3)3 + NH4OH 2. For the ionic chemical compounds listed in the table below, indicate whether they are soluble or insoluble in water. For insoluble compounds, indicate the colour of the precipitate. (See pages 45 and 54) Colour of Compound (if insoluble) Chemical Soluble or Insoluble in Compound Water? AgCl BaSCN
4. When a solutions of aluminum sulfate and potassium hydroxide are mixed, a precipitate forms. a. Write a balanced net ionic equation for the reaction. b. Calculate the mass of the precipitate when 3.89 g of aluminum sulfate in 100mL of solution is combined with 50 mL of the o.300 M KOH. c. What is the molarity of the ion in excess? (Ignore the spectator ions and assume that volumes are additive)
Write the (i) balanced conventional equation (CE), (ii) total ionic equation (TIE), and (iii) net ionic equation (NIE) for each of the reactions below. Include all state symbols. Assume that, if there is a reaction, it will go to completion. If there is no reaction, write "No Reaction" for the NIE but still complete the CE and TIE. a. Aqueous solutions of potassium sulfate and calcium iodide
Consider the following reaction: ___ HCl (aq) + ___ Ca(OH)2 (aq) ---> ___ CaCl2 (aq) + ___ H2O (l) . What is the coefficient in front of the water molecule, when the reaction is balanced to lowest whole number coefficients? A. 3 B. 1 C. 2 D. 4
3. Balance the reaction of sodium hydroxide and iron(II) chloride to give iron(II) hydroxide and sodium chloride, and then write the net ionic equation. Show states for all reactants and products (s, l, g, aq).
1. Aqueous copper (II) sulfate and 0.75 M sodium hydroxide react to form a precipitate of copper (II) hydroxide and aqueous sodium sulfate. Write the chemical equation for this reaction. Classify this reaction and write the general form for this type of reaction equation If both solutions were clear add the beginning of the reaction, why does this reaction form a blue solid precipitate? 2. Solid zinc metal reacts with aqueous hydrogen monochloride to form aqueous zinc chloride and hydrogen gas. Write the symbolic form of this chemical reaction. Classify this chemical reaction and write the general form of this type of reaction. What could we do to verify that the gas released was, in fact, hydrogen? Is zinc chloride soluble or insoluble in water? How do you know?
→ Fe(OH), (s) (bp) (bp) 82. Aqueous solutions of silver nitrate and potassium bromide react in a precipitation reaction to form insoluble silver bromide, as shown here: AGNO, (aq) + KBr (aq) → KNO, (aq) + AgBr (s) a. Rewrite this equation as an ionic equation. b. What are the spectator ions in this equation? c. Remove the spectator ions, and rewrite this as a net ionic equation. d. What is the driving force for this reaction?
33. You can -Text A 62.5 mL sample of a 0.118 M potassium sulfate solution is mixed with 37.0 mL of a 0.128 M lead(II) acetate solution and the following precipitation reaction occurs: The solid PbSO, is collected, dried, and found to have a mass of 1.00 g - Determine the limiting reactant, the theoretical yield, and the percent yield. ▸ Part A Part B Determine the theoretical yield. mass of PbSO, K₂SO, (aq) +Pb(C₂H₂O₂) (aq) +2KC₂H₂O₂ (aq) + PbSO,(s) ΗΘΕΙ ΑΣΦ Submit Previous Answers Bequest Answer nin * Incorrect; Try Again; 5 attempts remaining ? K