Lab 6 Alka Seltzer Strength_Spring2024

Name Lab Partner Section # Date Pre-Lab Assignment: Stoichiometry Lab 1. In a lab experiment similar to the one you are going to do, a student slowly added hy- drochloric acid (HCI) to an evaporating dish containing magnesium carbonate MgCO3. a. Complete and balance the following equation for the reaction between magnesium carbonate and hydrochloric acid. MgCO3 (s) + HCl (aq) → (aq) + H₂CO3(aq) (When writing the formula for the missing product did you consider the charges of the ions?) b. When carbonic acid is formed in a chemical reaction, it is unstable and immedi- ately decomposes into carbon dioxide and water. Rewrite the equation above to show the final products using this information.

A. REACTIONS OF HYDROCARBONS Three hydrocarbon samples were analyzed by various qualitative tests and the summary of their reactions is given in Table 1 below. Identify each unknown sample by matching the respective reaction profile with the given structures (A, B, or C). Table 1. Summary of Reactions of Hydrocarbon Samples Sample Brz in CCI4 KMNO, in NaOH AGNO3 in NH3 Fading of reddish- brown color Brown precipitates 1 No reaction Fading of reddish- brown color Brown precipitates Silver precipitates 3 Fading of reddish- No reaction No reaction brown color H3C `CH3 H,C CH3 А Sample Identity and Rationalization 1

If this item does not open automatically you can open Data Sheet here = 106106334 Part I. Reaction of Fe³+ and SCN™ Test tube A B C 5 Adding NH3 (aq) 1/1 Action performed Experiment 15 Chemical Equilibrium and Le Châtelier's Principle Adding Fe(NO3)3 (aq) Adding NaSCN (aq) Adding NaNO3(aq) Part II. Reaction of Cu²+ and aqueous NH3 Action performed Mixing CuSO4 and NH3 (aq). Oll y 31 88% + Data Sheet Observations Observations. DELL العال[ O : * 8 CH127 Introductory General Chemistry Laboratory Conclusion Conclusion O Dec 18 8:09 2 3 Р

A. REACTIONS OF HYDROCARBONS Three hydrocarbon samples were analyzed by various qualitative tests and the summary of their reactions is given in Table 1 below. Identify each unknown sample by matching the respective reaction profile with the given structures (A, B, or C). Table 1. Summary of Reactions of Hydrocarbon Samples   Sample Br2 in CCl4 KMnO4 in NaOH AgNO3 in NH3 1 Fading of reddish-brown color Brown precipitates No reaction 2 Fading of reddish-brown color Brown precipitates Silver precipitates 3 Fading of reddish-brown color No reaction No reaction           Sample Identity and Rationalization 1           2             3

maining Time: 1 hour, 01 minute, 27 seconds. uestion Completion Status: A Moving to another question will save this response. estion 33 For Questions 30-35: Nitric acid is prepared from the reaction of 69.0 grams of nitrogen dioxide with 36 grams of water. unbalanced chemical equation: NO2 + H₂O → HNO3 + NO How many grams of NO are produced? 60 g 45 g 30 g 15 g Moving to another question will save this response. 4 144

19. The chemical equation for photosynthesis is _CO2 (g) + _H₂O (1)→ __C6H1206 (s) + (C6H12O6 is glucose, the simplest sugar) a. Balance the chemical equation above by filling in the blanks. b. According to onetreeplanted.org, the average tree (across all climates and sizes) removes 10 kg of carbon dioxide from the atmosphere every year. Based on this, what mass of glucose is produced annually by the average tree? O2 (g) c. Teak is a common species of tropical tree. The graph below shows the amount of CO₂ absorbed by teak forests in tons of CO₂ per hectare of forest per year, according to the climate region where the forests are found (dry = low rainfall, humid=high rainfall). Looking at your photosynthesis equation again, what does this data suggest about which reactant is the limiting reactant for teak trees? Explain. C Teak Carbon sequestration rate (tons CO₂ ha -1yr -1) 10 10 20 Tropical humid Tropical dry Aboveground biomass, 0-20 years Belowground biomass, 0 -20 years

Mg + 2HCl → MgCl2 + H2 This experiment was performed two times. All values are valid to one decimal place. If the decimal place is not shown, add a ".0" Experiment Mass of Mg (mg) Starting Temperature (°C) Final Temperature (°C) 1 2 19.6 20.7 19.5 20.7 33 33.5 The previous page contained data from two experimental runs for the reaction between magnesium and hydrochloric acid. Mg+ 2HC! MgCl2 + H2 First, how many moles (n) of Mg reacted with the HCI? Use the average value of the two masses from your provided data set. Answer: 0.001658 I Mg + 2HCI MgCl2 + H2 Next, what is the amount of heat absorbed by the water (qsurr) in the experiment? Use the average AT from your data to calculate a single value for q. Report your answer in J. Remember to consult the lab manual and/or the video for any values you might need. Answer: Mg + 2HC! MgCl2 + H2 Finally, calculate A,H for this reaction and report your answer in kJ/mol. Answer:

Post- Lab Write the correct formula of the products and balance each equation. A. Instructor Demonstration- Combination reaction Reactants Products Mg (s) + O, (g) Magnesium oxide (s) Balanced equation:

12. Name each chemical and complete the reaction ↑ Add file + H₂O

CHEMISTRY 1110L LAB REPORT: REACTIONS OF COPPER (Part B) 1. Reaction 4: a. Color of copper(II) sulfate b. Water solubility of copper(II) sulfate 2. Reaction 5: CuO + H₂SO4 → CuSO4 + Zn →>> - 5. Percent recovery (calculations) 3. Mass of copper metal recovered 4. Initial mass of copper (from Part A) CuSO4 + Cu + ZnSO4 + Zn + H₂SO4 a. Color of zinc metal (before reaction) b. Color/appearance of copper metal (after reaction) c. Color of solution before reaction d. Color of solution after reaction e. Color of hydrogen gas ZnSO4 H₂O blue Solid Water 6. Initials of instructor or teaching assistant (TA) own H₂ Name • Loona Alg busi Partner Desk # AR Solid metal-normal color 20

IDENTIFYING SYNTHESIS REACTIONS GAOW Tên equations are listed below. Some are synthesis reactions, Some are not. Make a check (/) in the correct box next to each equation. Not a Equation Synthesis Reaction Synthesis Reaction 1. 2K + Br, – 2KB1 2. 2H,0 2H, + O, - 3. Nacl Na + Cl 4. 4Au + 30, 2Au,0, 5. 2Na + 2HCI → 2NACI + H, Cu + Br, CuBr, > 7. Zn + S ZnS 8. 2NA + Br, → 2NAB. 9. 2H8O 2Hg + O, > 10. 2Na + 1, 2Nal 6.

Given the combustion reaction below, how many moles of CO2 are formed given that you start with 1.50 x 10^-2 mol of C3H8O. (Assume O2 is in excess).  2 C3H8O + 9O2 ---> 6 CO2 + 8 H2O A. 3.00 x 10^-2 mol B. 4.50 x 10^-2 mol C. 5.00 x 10^-3 mol D. 7.50 x 10^-3 mol E. none of the above

Chemical Reactions and Equations 3. Observation of burning match or splint. What caused the change in the burning match or splint? 4. Na,CO3(s)+ HCl(aq) » CO, (g)+ H2O(1)+ NaCl(aq) 5. Type of reaction: F. Hydrogen Peroxide Reactants 1. Appearance of Reactants 2. Evidence of a Chemical Reaction H,O2(aq) 3. H2O¿(aq) – KI H2O(1) +. O2(g) 4. Type of chemical reaction: Questions and Problems Q1 What evidence of a chemical reaction might you see in the following cases? Refer to Table 1. a. dropping an Alka-Seltzer tablet into a glass of water b. bleaching a stain c. burning a match d. rusting of an iron nail Q2 Balance the following equations: a. Mg(s) + HCl(aq) H2(g)+. MgCl2 (aq) b. Al(s) + 02(g) Al,O;(s) 89

O Launch Meeting - Zoom O Launch Meeting - Zoom od212ou%3D2591470&isprv &drc3D1&qi=24592388cfql%=D08drnb- ttempt 1 A honeycomb-shape casing of the metals platinum (Pt), rhodium (Rh), and palladium (Pd) in catalytic converters of automobiles cause more reactions to take place that produce less harmful gases without being affected by the reaction. These metals are catalysts because: They cause the reactions without being affected. They are formed into a honeycomb shape. They are metals. They help produce less harmful gasses.

2 Fe + Oz →2 FeO 1. The chemical in the pink box is a... A. subscript B. coefficient C. reactant D. product 2. The number in the green box is a... A. subscript B. coefficient C. reactant D. product

Which of the following statements is true? (Several options can be specified.) a.The stoichiometric coefficient of a compound is the number in front of the compound in the reaction formula. The coefficient is negative for a reactant and positive for a product.b.Reaction heat is the heat development that occurs during a chemical reaction.c.When a gas is heated, the enthalpy content decreases.d.Entalpine changes during phase transformation (for example when iron melts or water evaporates).e.In an endothermic reaction, heat develops.

Complete the ICF (BCA) table below for the hypothetical chemical reaction. All values are in moles. Enter all values with three digits (like shown) and include negative or positive signs for the "Change" row. A + 2B 3C + D. INITIAL CHANGE FINAL A 5.00 4.00 B 2.00 0.00 C 0.00 D 0.00

Balance the following reaction in your notes, assuming basic conditions (use the smallest whole number coefficients): Mn²+ (aq) + CIO (aq) → CIO₂(g) + MnO₂ (s) Then use the controls below to enter your equation and check your answer. Reactants Add Reactant Products Add Product Preview: Evaluate

Balance the reaction shown below:   H2CO3+NaOH→Na2CO3+H2OH2CO3+NaOH→Na2CO3+H2O  Once balanced, given 0.367 moles H2CO3H2CO3, calculate the grams of H2OH2O produced. A. 1.65 B. 38.3 C. 13.2 D. 61.8 E. 16.9

Based on the process below, how many moles of electrons are transferred during the reaction? 3Pb(s) + 2Cr3+ (aq) = 3Pb²+ (aq) + 2Cr(s) n = [?] moles of e- moles of electrons Enter Copyright © 2003-2022 International Academy of Science. All Rights Reserved.

Which of the following is always correct in considering the percentage yield of a reaction?     There are cases that percentage yield is greater than 100%. There are cases that percentage yield is greater than 100%. Theoretical yield is always greater than actual yield. Theoretical yield is always greater than actual yield. There is no relationship between actual and percent yield. There is no relationship between actual and percent yield. Percent yield is derived from pre and post lab experiments. Percent yield is derived from pre and post lab experiments. Actual yield is always greater than theoretical yield.    Which of the following is always correct in considering the percentage yield of a reaction?     There are cases that percentage yield is greater than 100%. There are cases that percentage yield is greater than 100%. Theoretical yield is always greater than actual yield. Theoretical yield is always greater than actual yield. There…

Predict he products and balance the chemical equation involving decomposition reaction. Have photo of your answers and attach it at the box below. Accepts pdf and jpg only. Use a darker pen. Decomposition Reaction 1. Fe,0, 2. Sodium chlorate 3. Magnesium carbonate 4. MgSO4, 7 H,0 5. NaHCO, Single Displacement Reaction 1. Na + Cas 2. Li + Bao| heat 3. Ва + H,0

A LEAP 2025 Prep in 8th Grade Sci x s.com/r/s/0/doc/607216/sp/179325173/mi/571531285?cfi=%2F4%2F4 Chapter 7 Key Terms Activity Word Bank covalent ionic atoms ions reactants molecules bonding gains products share cation equation reaction anion form 2. or compounds through 3. during a chemical 4. The best way to express this reaction is with a chemical 5. In this expression, you can show how 6. result into 7. Some of the reactions involve 8, in which a(n) and a(n) 10. form a neutral product. The atoms form 9. bonds in which one atom 12. an electron and another 11 atom 13 an electron, 14 bonding occurs when atoms 15. electrons. Key terms are defined in the book's glossary. Answers to Key Term Activities and chapter reviews are found in the Teacher's Cuide Teachers, remember there is a review test for your use in the Teacher's Guide hp

What is the missing particle in the reaction below? 27/13 Al +1/1 H → 27/14 Si + ?   A. e   B. n   C. He   D. H

Using your reaction page, predicte the products and balance the reation. What type of reaction would the following be ID as? KCI(aq) + NaNO3(ag) →? Comb. #1 no reaction Comb. #4 Comb. #2 Double Replacement Decomp. #5 Single Replacement #1 Decomp. #2 Decomp. # 1 Single Replacement # 2 Total Combustion of a Hydrocarbon Comb. #3 Decomp. #4 Decomp. #3 hp C %23 %24 % & 3. 4 8 9. AU S d. m OO00 O O O O O O O O

Please help me how to solve this equation. Thank you very much.

Balance the following chemical equation by placing a coefficient (including 1) in each answer box that is in front of each reactant and each product. While coefficients that are equal to 1 are not placed in front of either a reactant or product, you MUST include any coefficient that is equal to 1 in this problem. type your answer... C₂H12 + type your answer... 2 type your answer... CO₂ + type your answer... H₂O

In part 1 of this lab, you will be calculating A₁H by conducting constant-pressure calorimetry measurements. One of the final steps in this calculation is obtaining ArH by taking the q value (with respect to the system) and dividing by n. What number of moles (n) will you be using in the above formula? Select one: Number of moles of magnesium, since Mg is in the balanced chemical equation and is a part of the system Number of moles of water

Predict the products of the reaction below. That is, complete the right-hand side of the chemical equation. Be sure your equation is balanced. HI + NaOH → I Don't Know 1841 Submit 3 E 5 T 6 G 0-0 X S stv♫ 5 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Cer A all 9 zoom

2 Fe + Oz→2 FeO The chemical in the pink box is a... A. subscript B. coefficient C. reactant D. product The number in the green box is a... A. subscript В. соefficient C. reactant D. product The numbers in red boxes are... A. subscripts В. соeficients C. reactants D. products The chemicals in the purple box are... A. subscripts В. соefficients C. reactants D. products

What is the molar mass of each of the following compounds? Show all work.a. Ru(NH3)6Cl3b. WO2c. PbI2

CABOR Page 12 > ar65 ZOOM Learning Check Balance each equation. А. Mg(s) +__N2(g) →_M93N2(s) В. Al(s) +_Cl,(g) →_AICI3(s) BF3(g) +_H20(1) →_B203(aq) +_HF(aq) D. Fe203(s) +__C(s) _Fe(s) +__CO2(g) E. Al(s) + Fe0(s) _Fe(s) +_Al,03(s) 184 RO DE G B. LL C.

How many moles of W are needed to react with 1.0 mol of Ho in the hypothetic chemical reaction? 3W + 2Ho  →  2W3Ho   a. 0   b. 1.5   c. 2   d. 3   e. 1