Part FThe third variable (call it v) is v=x1-cx2 + x3, where c is a constant you need to determine so that the equation for v is theSHM equation. Determine v. The solution to the equation for vis v = 2B cos(t + b).Express your answer in terms of some, all, or none of the variables 21, 22, 23, and the appropriate constants.v =ΜΕ ΑΣΦSubmitRequest Answer?

Step 1:To determine the constant c such that v=x1-cx2+x3 represents the SHM(simple harmonic motion)…

Answered: Part F The third variable (call it v)…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.54QE

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A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.
Insoluble AgCl(s) precipitates when solutions of AgNO3(aq) and NaCl(aq) are mixed. AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) rH = ? To measure the energy evolved in this reaction, 250. mL of 0.16 M AgNO3(aq) and 125 mL of 0.32 M NaCl(aq) are mixed in a coffee-cup calorimeter. The temperature of the mixture rises from 21.15 C to 22.90 C. Calculate the enthalpy change for the precipitation of AgCl(s), in kJ/mol. (Assume the density of the solution is 1.0 g/mL and its specific heat capacity is 4.2 J/g K.)
The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
Write a balanced equation for the combustion of propane. (Be sure to include states of matter in your equation.) x | x. | He (aq), | 5. H,0(g) Co, (g) +
(f) The student finds the following particulate model of AgCl(s). Assuming the crystal structures are similar, how should the student modify the model to represent AgBr(s)? Justify your answer in terms of the radius and arrangement of electrons in the ions. CI- Ag+ CIF Ag* 口 Ag+ CI- Ag* CIT CI- Ag+ CI- Ag+ Ag+ CI- Ag+ CIT
Given the following data: FEE Conc. (M) Volume (mL) Tinitial (°C) Tfinal (°C) Solution NaOH 0.750 50.00 19.84 23.18 HCI 0.500 50.00 19.84 Calculate AH° for the reaction: HCl(aq) + NaOH(aq) H2O(1) + NaCl(aq) You may assume all solutions to have the same density and specific heat as water (1.00 g/mL and 4.184 J/g°C) kJ/mol
Equations: -Σ (n . ΔΗμoduats) -Σ (n - ΔΗ, ΔC Σ (n . ΔGproducts ) Σ (n . ΔΕreac tan ts, ΔΗ Ireac tan ts) AS = £ (n · ASproducts) – E (n · ASreac tan ts ) AG = ΔΗ-ΤAS The reaction for the decomposition of calcium carbonate is given below. Using the given table of values, calculate AH°, AS°, and AG° at 25 °C. СаСОз (s) — СаО (s) + CO2 (g) AS (K) kJ J kJ ΔΗ AG ( mol mol·K mol CaCO3 -1206 92.9 -1128.8 CaO -634.9 38.2 -604.04 CO2 -393.5 213.8 -394.4 4 7 8 9. 10 11 12 13 前Review
Calculate Kpfor the reaction 2NOCl(g) -> 2NO(g) + Cl2(g) at 400°C if Kcat 400°C for this reaction is 2.1 × 10–2.
2H,O1) = H3O+(aq) + OH (aq) Kw = 1.0x 1014 at 25 °C Kw=5.5x 1014 at 50 °C Based on this data, which statements are true? You may check any combination of statements. 2H20(1) = H3O*(aq) + OH(aq) is an exothermic reaction 0.10 M NAOH solution at 50°C has pH = 12.26 Pure water at 50°C contains more ions than pure water at 25 °C.
We want to calculate the heat of dissolution of sulfuric acid in water. There is a calorimeter with Cequipo = 4.5 Kcal / ° Cand with 3 liters of water in the jacket. Put in the reaction chamber of the calorimeter 4 liters of water and 2 liters of 2 Normal sulfuric acid and density 1.2 g / ml. The cp of the resulting solution is 1.2 cal / g°C (water + sulfuric acid). It is known that 35% of the heat produced by the solution goes to the environment. The total system undergoes an increase of 5° C. Calculate the heat of dissolution of sulfuric acid in water in Kj / mol of sulfuric acid. a. +200.44 Kj/mol b. -204.44 Kj/mol C. -244.05 Kj/mol d. -255.05 Kj/mol
3a. CO₂ can be formed by: BaCO 3 (s) + 2H+¹ (aq) Ba→ܢ +2 (aq) + H2O(liq) + CO2(g) Write the thermodynamic equilibrium constant expression. (4 pts) 3b. K = 3.72 × 10+9 at 1 atm and 298 K. Find AG° in kJ. Show all units and conversion factors. Use significant figures. (4 pts)
Suppose that 125 mL of 0.1125 M HCI is reacted with 155 mL of 0.1010 M NaOH in a coffee-cup calorimeter. HCl(aq) + NaOH H20(1) + NaCl(aq) -56 KJ mol ΔΗ If the initial temperature of the mixture is 22.1°C, calculate the final temperature of the mixture given the following information. Ssolution = 4.1 g.°C %3D Dsolution = 1.02 mL 25.5 °C 24.3 °C 22.8 °C O 19.8 °C

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