(f) Why alternating current is used for conductometric measurements? (g) What will happen if large quantities of indicator solution are used for the determination of pH by color matching? (h) What is the best way to ascertain that a reaction is first order?

(f) Why alternating current is used for conductometric measurements? (g) What will happen if large quantities of indicator solution are used for the determination of pH by color matching? (h) What is the best way to ascertain that a reaction is first order?

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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In a coffee-cup calorimeter, 110.0 mL of 1.2 M NaOH and 110.0 mL of 1.2 M HCl are mixed. Both solutions were originally at 22.5°C. After the reaction, the final temperature is 30.5°C. Assuming that all the solutions have a density of 1.0 g/cm³ and a specific heat capacity of 4.18 J/°C.g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. AH = 0.182 kJ/mol
When HCI(aq) is added to calcium carbonate solid, carbon dioxide gas, liquid water and aqueous calcium chloride form: CaCO3(s) + 2HCI(aq) → Co,(g) + CaCl,(aq) + H,0(1) This reaction is used by geologists to confirm the presence of limestone (calcium carbonate) in minerals. In this experiment you are trying to determine the effect of concentration of HCI(aq) on the production of carbon dioxide. a. Based upon the information above, come up with a question to answer. (C:1) You can use the following equipment to answer this question: calcium carbonate chips, 1.90 mol/L HCI(aq), pH meter (measures hydrogen ion concentration), beaker, timer, apparatus to measure gas produced b. Based upon the equipment provided above, design a procedure to answer your question. Ensure you provide numbered steps. (1:3, C:2) c. Hypothesize an answer to your question. (I:1) Give reasons for your hypothesis. Ensure you are very specific. (A:3) From your experiment, you collect the following data:
24. A 500-cm^3 sample of1.0 M NaOH(aq)is added to 500cm3 of 1.0M HCl(aq)in a Styrofoam cup, and the solution is quickly stirred. The rise in temperature (AT1) is measured. The experiment is repeated using 100cm^3 of each solution, and the rise in temperature (AT2) is measured. What conclusion can you draw about AT1 and AT2? HCl(aq)+NaOH(aq) H2O(1)+NaCL(aq); AH∞=-55.8KJ a. AT1 is five times as large as AT2 b. AT1 is less than AT2 c. AT2 is greater than AT1 d. AT2 is equal to AT1 e. AT2 is five times as large as AT1
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(a) Draw a Lewis diagram for carbonic acid, H,CO3, with a central carbon atóm bonded to the three oxygen atoms. (b) Carbonic acid is unstable in aqueous solution and converts to dissolved carbon dioxide. Use bond enthal- pies to estimate the enthalpy change for the following reaction: H,CO;→ H,O + CO,
0.5Ν2 (NH3 (g) H2 (g) + 1.5H2 (g) +1.2502 (g) (g) +0.502 (g) → NH3 (g) NO 2NO H2O (1) (g) (g) ΔΗ1° Use the data from the table above to determine AH° for the reaction below, expressed in terms of ΔΗ1°, ΔΗ2°, and ΔΗ3°. N2 (g) + O2 (g) + 1.5H2O (I)|ΔΗ2° ΔΗ3°
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
When 50 mL of 0.400 M aqueous hydrochloric acid (HCI; Molar mass: 36.5 g'mol) is mixed with 50 mL of 0.400 M aqueous sodium hydroxide (NaOH; Molar mass: 40 g/mol) in a calorimeter the temperature increases by 3.4°C. If the heat capacity of calorimeter (excluding water) is 320 Ji°C, calculate AH of neutralization reaction in kJ/mol. (Specific heat capacity of water is 4.184 J°C- gl. Density of water is 1 g'mL Assume that the heat capacity and the density of the solution is same with water) 2511 kJ/mol O A. 1.09 kJ/mol O B. 1088 kJ/mol OC. 125.5 kJ/mol OD. 2.5 kJ/mol O E.
Using the equations H₂ (g) + Cl₂ (g) → 2 HCI (g) AH° = -184.6 kJ/mol C (s) + 2 Cl₂ (g) →→ CCI (g) AH° = -95.7 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction C (s) + 4 HCI (g) → CCI (g) + 2 H₂ (g). 4 2