580368 Determining the Ksp of Calcium Hydroxide Q

The reaction A(g) + 2B(g)    C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate Kc for this reaction. Round off the answer to two significant digits. Group of answer choices 0.060 5.1 17 19 25

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

cem 5 5 Constants I P Part A The concentration of Br in a sample of seawater is 3.3 - 10 M. If a liter of seawater has a mass of 1.0 kg, the concentration of Br is ppm. O 3.3 O 0.33 O 0.0033 O 26 O 0.026 Submit Request Answer

Based on your ICE table (Part 2) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ка = = 3.2 × 10-9 RESET [0] [0.110] [0.220] [0.101] [0.229] [0.106] ☑ (x)] [2x] [0.110+x] [0.110-x] [0.220 + x] [0.220-x] [0.101 + x] [0.101 - x] [0.229 +x] [0.229-x] [0.106 + x] [0.106 - x] < PREV 2 3 Based on your ICE table (Part 2) and the equilibrium expression for Ka (Part 3), determine the pH of solution. pH = RESET 0 20.3 2.03 8.85 5.15 1.41 × 10-* 7.09 × 10-€ 0.110 0.958 1.96

According to the Arrhenius equation, what does the slope of the line on this graph represent? In(k) vs 1/T -5 -50200315 0.002 0.00325 0.0033 0.00335 0.0034 -5.4 + -5.6 y = -9253x + 24.504 25.8 -6 -6.2 -6.4 -6.6 -6.8 1/T a) 24.504 Ea b) -9253 = LnA c) -9253 -Ea d) -9253-Ea/R =

For each of the following reactions, indicate if there is something wrong with the reaction. If something is wrong, say what it is.a) 2H2(g) + O2(g) 2H2O(l)b) C(s) + H2O(p) CO(g) + H2(g)c) N2(g) + H2(g) NH3(g)d) Cℓ2O7() + H2O(l) 2HBrO4(aq)

Determine the pH of a solution of aspirin (acetylsalicylic acid, HC,H7O4) by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka of aspirin is 3.3 × 104. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT 652 mg of aspirin (HC9H7O4) is dissolved in an aqueous solution of 237 mL aqueous solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. HC9H7O4(aq) + H₂O(1) Initial (M) Change (M) Equilibrium (M) ☐ 0 = H3O+(aq) + C9H7O4(aq) 2.75 x 10-3 3.62 × 10-3 1.53 x 10-5 15.3 0.0153 RESET +x -x 2.75 x 10-3 + x 2.75 x 10-3-X 3.62 x 10-3 + x 3.62 x 10-3-X 1.53 x 10-5 + X 1.53 x 10-5-x 15.3 + x 15.3 - x 0.0153 + x 0.0153 - x

Based on your ICE table (Part 2) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = 2.9 × 10-8 RESET [0] (0.13] [0.37] (0.010] [0.040] [0.10] [0.40] [x] [2x] [0.13 + x) [0.13-x] [0.010+x] [0.010-x] [0.040 + x] [0.040 - x] [0.10+x] [0.10-x] [0.40+x] [0.40-x] PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Ka (Part 3), determine the pH of solution. pH = RESET 0 7.3 × 10* 5.86 18.74 1.4 × 10+ 0.13 8.14 0.89

Problems 34 and 35 are about the exothermic reaction of iodine with iodide ion shown below. 1₂(aq) + I-¯(aq) 13¯(aq) Keq = 750 (at 25 °C) 34. 1.0 × 104 mol I₂ and 4.0 × 10-³ mol KI are dissolved in water at 25 °C to give 100.0 mL of solution. What is the equilibrium concentration of I₂ in this solution? (A) 1.3 x 10-6 M (C) 5.0 x 10-4 M (B) 3.4 x 10-5 M (D) 5.3 x 10-3 M 35. Which changes will result in an increase in the number of moles of I₂(aq) present at equilibrium? I. Increasing the temperature II. Replacing the KI with an equal mass of Nal (A) I only (C) Both I and II (B) II only (D) Neither I nor II

Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = = 1.8 × 10-5 [500.0] [0.200] RESET [5.00] [1.0 × 10-9] [1.0 × 10-9] [1.8 × 10-5] [x + 5.00] [x + 1.0 × 10] [x-1.0 x 10 x + 1.0 × 10-] [x-1.0 × 10-] [x+1.8 × 10] [x-1.8 × 10%] [0] [x-5.00] < PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression, Ka (Part 2), determine the original mass of solid CH3COONa added to create this buffer solution. MNACH3COO g 0 0.360 30 21 43 11 15 36 x 10' 59 x 105 43 x 105 RESET 59 50

Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ка = RESET [0] [0.95] [0.68] [8.68] [x] [2x] [2x]² [0.95+x] [0.95 - x] [0.95 + 2x] [0.95 -2x] [0.68+x] [0.68 - x] [0.68 + 2x] [0.68 - 2x] 8.68 0.939 4.79 × 10-* 2.09 × 10-º < PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Ka (Part 2), determine the pH of the buffer solution. pH RESET 0 19.65 5.46 0.95 0.022 8.53 3.4 × 10-€ 2.9 × 10-9

I need help with the expel nation for question 7 please!

AutoSave On O 2OB Chapter 10 homeworkcomplete Saved 9 Search Julianna Wren JW File Home Insert Draw Design Layout References Mailings Review View Help B Share Indicate how each of the following will affect the equilibrium concentration of H20 in the reaction: increase, decrease, or no change 2HF(g) + O,(g) + 76 kcal S H,O (g) + OF2(g) a. Adding more OF2 (g) b. Increasing the temperature c. Increasing the volume of the container С. d. Decreasing the volume of the container Adding a catalyst е. D, Focus 8:53 PM Page 4 of 4 560 words 47% 11/14/2020 e Type here to search Prisc F10 F9 F8 FS F6

Consider the reaction below. If the initial concentration of CO2 was 0.500 M and the initial concentration of NH3 was 0.750 M, calculate the equilibrium concentration of urea (CO(CH2)2). CO2 (aq) + 2 NH3 (aq) CO(NH2)2 (aq) H20 (1) Ko = 3.54 x 10-8

# 3 E D C Energy diagrams for two reactions are shown. Macmillan Learning Energy (kJ/mol) e 150 100 50- What is the heat of reaction for Reaction A? AHrxnA = 4 FER 20 What is the activation energy for Reaction A? R F V Reaction progress Reaction A 5 T G Search or type URL G B tv 6 MacBook Pro Y Ⓒ H 201 7 N U S J kJ mol 00 8 M I Energy (kJ/mol) 150 T 100- NIMZAO ✪ 50 What is the heat of reaction for Reaction B? AHxnB = What is the activation energy for Reaction B? K ( - O 9 < O I * ) -C O Reaction progress Reaction B L command ») P . V = : P W ; 242) { option [ SEC e = ? O kJ mol 1 delete retu

Time (min) 0.5 1 15 2 2.5 3 4.7 [Z] (mg/mL) 1 0.66 0.5 0.4 A. 5.1 B. 7.5 C. 9.5 D. 19.5 E. 14.8 0.334 0.286 0.192 From time zero, how long (in min) will it take for the drug's concentration to drop down to 0.05 mg/ml? (Hint: While you can, you do not have to calculate Co to answer this question) Rationale (YRI Chemical Kinetics and Drug Stability: Calculations: Please refer to calculations of the variou

2NH3(g) 26. Which of the following statements is true about the I.C.E. table below for the reaction: 3H2(g) + N2(g) at a given temperature. 3H2(g) N2(g) 2 2NH3(g) 0.24 M 0.52 M C E 0.84 M S a) y = + 0.60 M b) z = + 0.80 M c) t = + 0.12 M d) s = + 0.80 M e) none of the above

a *ACTIVITY 6.pdf O File D:/1st%20sem/chemistry%201/activity%20chem/ACTIVITY%206.pdf + O O CE Page view A Read aloud O Add text V Draw E Highlight O Erase of 2 Republic of the Philippines Laguna State Polptechnic University Province of Laguna ISO goos a015 Certified Level l Institutionally Accredited ACTIVITY TASK Activity 6 State the type of Chemical Reaction 1. BaCl, + H,SO → 2. CH12 + O2→ 3. Zn + CuSO,→ 4. Cs + Br, > 5. FeCO, → 1SPU SELE-PACED LEARNING MOnuLE: PHYSICAL SCIENCE P Type here to search 29°C Mostly cloudy A 回 ENG 4:55 pm 28/10/2021

60 50 40 kcal/mol 30 20 10 course of rx The reaction requires a constant input of energy to proceed A. True B. False Reset Selection

a) HJinitinl Rate in M-s 2.5 x 10 Experiment initial 1 0.0020 M 0.0050 M 2 0.0020 M 0.0025 M 1.3 x 10 0.0015 M 0.0025 M 1.3 x 10 4. 0.0050 M 0.0010 M 0.5 x 103 According to the experimental data and by considering the reaction given below, find and demonstrate the way to calculate the rate law. Explain each step. Initial rate data: 2H,(g) + Cl{g) –→ 2HCI(g) b) Consider this reaction. 4NH,(g) + 30,(g) 2N{g) + 6H,O(!) If the rate of formation of N, is 0.10 M-s, what is the corresponding rate of disappearance of O,? Explain step by step how to calculate the target value.

Part 1: Making Sandwiches: O Cheese 4 slices 1) The is a simulation of a two-reactant synthesis reaction. 2) Take some time and familiarize yourself with the simulation. 6 slices 8 slices 3) Set the reaction to a simple mole ratio of 2:1:1 4) Complete the table below while making tasty cheese sandwiches: Bread Used Cheese Used 2 slices 3 slices 28 02 5 AD Reactants PRE 5 2 3 Sandwiches Made Products 5 sandwiches 4 sandwiches Leftovers

e HW 11/10 ormat Tools Add-ons Help Last edit was 5 minutes ago BIUA Normal text Helvetica... 11 2 3 Which letter correctly labels the reactants in the chemical reaction? 4AI + 302 2 Al203 C A. A В. В С. С

The graphs below show the relative concentration of N₂O4(g) and NO2(g) as various stresses are exerted on the equilibrium system N₂O4(g) + heat 2 NO2(g). (Note: The graphs are not drawn to scale.) Graph M Concentration (mol/L) Concentration (mol/L) Graph N Graph M Graph P N₂O4(2) Graph O NO 20 Reaction coordinate N₂OA NO2(g) Graph O Reaction coordinate 1. 2. 3. Concentration (mol/L) Match each of the graphs with the appropriate stress. 4. Concentration (mol/L) N₂O) NO ₂0 Reaction coordinate N₂O) NO 21 Graph N Graph P Reaction coordinate removing NO2(g) cooling system adding heat adding N₂O4(g)

Activity 1: Complete Me! Direction: Complete the following table. Write your answer on a separate sheet of paper. Equilibrium Reaction Effect Keq expression Stress Equilibrium shift (encircle your answer) Forward applied (encircle your answer) Ha + Cla = | 2HCI Decreasing the pressure (increase, decrease, no change) in the number (HCIJ Keq - Backward No Shift of moles of HCl(g) (increase, decrease, no change) in the volume of Increasing Fe,O +4 Ha + heat 2 Forward Keq = the Backward 3Fe + 4H,O temperature No Shift water vapor collected of (increase, decrease, no change) the number of moles of NO 2NO + Oz 2NO + heat Forward Backward No Shift Addition (NO,P |NO]F|0,]| Keq = helium Forward H,CO» = CO2 + H,O Removal of (increase, decrease, no change) in the amount Keq - (H,CO, CO2 Backward No Shift of H,CO, (increase, decrease, no change) in amount of o, (increase, the volume of decrease, no change) in the Increasing the Forward Backward No Shift Keq= temperature the 4 NH3%g + 502 2 4NO+ 6…

O The reaction rate decreases. What mass of NaCl in grams is needed to prepare 2,500 g of 1.5% (m/m) NaCI solution? * 380 g NaCl O 38 g NaCl O 1.67 g NaCI 3.8 g NaCI You add solute to a solution and notice that all the solute crystallizes. The origin solution was

For the reaction: 2 H2(g) + O2(g) = 2 H20(g) at a certain temperature the Keg is 1.8x105 If the concentrations in a reaction vessel at a given time are [H2] = 3.0 mol/L, [02] = 2.0 mol/L and [H,O] = 0.010 mol/L, which of the following statements is true? %3D %3D %3D The system is not at equilibrium, the reaction will proceed to the left O The system is at equilibrium since Q = K O The E, for the forward reaction is very large The system is not at equilibrium, the reaction will proceed to the right

MISSED THIS? Watch KCV 13.4; Read Section 13.4. You can click on the Review link to access the section in your e Text. Review | Constants | Periodic lable 100 Part A 90 A KCl solution containing 44 g of KCl per 100.0 g of water is cooled from 70 °C to 0 °C. What happens during cooling? 80 - NaNO 70 O At 70 °C the solution is unsaturated, but by 0 °C the solution is saturated; therefore a precipitate will form. 60 - NaSO4 O At 70 °C the solution is supersaturated, but by 0 °C the solution is unsaturated; therefore no precipitate will form. 50 - KCI At 70 °C the solution is supersaturated; therefore a precipitate will form upon cooling. 40 - O At 70 °C the solution is unsaturated, and at 0 °C the solution is also unsaturated; therefore no precipitate will form. NaCl 30- Request Answer KdO, Submit 20 - 10 - 0- Provide Feedback 10 20 30 40 50 60 70 80 90 100 Next > Temperature (°C) Solubility (g solute in 100 g H¿O) CaCl Pb(NO,)2 KNO3 KCrzO,

The radioisotope phosphorus-32 is used in tracers for measuring phosphorus uptake by plants. The half-life of phosphorus-32 is 14.3 days. If you begin with 40.4 mg of this isotope, what mass remains after 22.3 days have passed?_____mg 42.0 mL sample of a 0.476 M aqueous hydrofluoric acid solution is titrated with a 0.305 M aqueous barium hydroxide solution. What is the pH after 19.9 mL of base have been added? Ka for HF is 7.2 × 10^-4 pH =____

CollegeBoard AP Classroom A UPDATES AVAILABLE Unit 9 Progress Check: MCQ Do you want to install the updates now? 8 9 10 11 13 Reaction 1: X2Y 30 Reaction 2: K undergoes the two competing reactions represented above. The following graph shows the changes in energy that occur as the two reactions take place. Y Reaction 1 Reaction 2 Reaction Coordinate In an experiment done at a low temperature, one hour after the reaction started, Y was produced but almost no Z was produced. At a much higher temperature, one hour after the reaction started, both Y and Z had been produced. Which of the following best explains why very little Z was produced at the lower temperature? O Search or enter website name Energy

Chem 11- Chemistry for Engineers 66 s Choose the correct reactants for the double displacement equation below. - K2SO4 + Fe(OH)3 a) FeSO4 + K2(OH)3 b) Fea(SO4)2 + KOH c) Fez(SO2)a + KH d) Fea(SO4)a + KOH 6. Balance the equation above with the correct reactants. a) 1, 2, 1, 2 b) 1, 2, 3, 2 c) 1, 6, 3, 2 d) 1, 6, 1, 2