Sodium reacts violently with water according to the equation:2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g)The resulting solution has a higher temperature than the water prior to the addition ofsodium. What are the signs of AH° and AS° for this reaction?C) AH° is positive and AS is negative.A) AH° is negative and AS° is negative.OB) AH° is negative and AS° is positive.D) AH° is positive and AS° is positive.

Explanation: ΔS° is negative (ΔS° < 0) and the sign of ΔH° is also negative (ΔH°…

Answered: Sodium reacts violently with water…

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

Vinegar (chemical name : acetic acid, CH3COOH) is a weak acid. Consider the ionization of acetic acid in water. CH3COOH(aq) = H*(aq) + CH3COO (aq) Kc=6.80 ×10-4 If the initial concentration of acetic acid is 0.150 M. What is the concentration of hydrogen ions (H*) at equilibrium? O 0.0100 M O 0.0500 M O 0.100 M O 0.500 M
When 0.0500 mol of HCl(aq) reacts with 0.0500 mol of NaOH(aq) to form 0.0500 mol of NaCl(aq), 2.9 kJ of heat are produced. What is ΔH, the enthalpy change, per mole of acid reacting, for the acid-base reactionrun under the conditions described as given below?
:(((((((
5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.
In the following acid-base equilibria of weak acids in water, label the acid (A), the base (B), the conjugate acid (CA), and the conjugate base (CB). HCIO,(aq) + H,O(l) = H,O*(aq) + ClO, (aq) ******* H₂CO3(aq) + H₂O(1) = H₂O+ (aq) + HCO3(aq) H₂O(1) + CH3NH3(aq) → CH3NH₂(aq) + H₂O+ (aq) O $0 CH3COOH(aq) + H₂O(1) ⇒ CH₂COO¯(aq) + H₂O+ (aq) Answer Bank CA CB
Explain about Rapid acid–base reactions? When it occurs ?
For the following equilibrium reaction: NaOH(Aq) + HCl(aq) HOH(aq) + NaCl(aq) + Δ What happens if you add: A) KCl B)KBr
Suppose you add a few drops of ammonia into a bucket of water. Then you add a couple of drops of phenolphthalein into the bucket. The color of the water becomes pink or red. Now you have a weird idea. If you spray that colored water on to the white clothes of your friends, they will be very annoyed. What will be the color of the clothes after a few minutes? Explain.
Part A Water ionizes by the equation =H+(aq) + OH (ag) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H*] and [OH ]: What is the H† concentration for an aqueous solution with pOH = 2.73 at 25 °C? Express your answer to two significant figures and include the appropriate units. Kw = [H*][OH¯] • View Available Hint(s) Keep in mind that, like all equilibrium constants, the value of Kw changes with temperature. ? [H*] = Value Units
Acetaldehyde (CH3CHO) is an important chemical both industrially and biologically. For instance, it is a (somewhat toxic) intermediate in the body's metabolism of ethanol into acetic acid, and thus is possibly implicated in the "hungover" symptoms of someone who has had too much to drink the night before. In aqueous solution, it establishes an equilibrium with a hydrated form, shown below. CH3CHO (aq) + H2O (l) <--> CH3CH(OH)2 (aq) You start with an aqueous sample, already at equilibrium, with the CH3CH(OH)2 (the hydrated form) at a concentration of 2.60 M. You have no information about how much, if any, of the anhydrous form (CH3CHO) is initially in the flask. If you add 2.0 M of CH3CHO to the reaction flask, and as the equilibrium is being restored the amount of CH3CH(OH)2 changes by 1.13 M, what is the final amount of CH3CHO?
8 ) can you help me solve this
From the information given below, select the acid which would have the lowest pOH value. All solutions have 0.100 M at 25.0 °C. Acid #1: pH = 3.07 Acid #3: pH = 2.74 Acid #4: K₂= 7.3 x 10-6 Acid #2: K₂= 3.5 x 10-5

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS