Write balanced complete ionic and net ionic equations for each reaction. a. HI ( a q ) + KOH ( a q ) → H 2 O ( l ) + KI ( a q ) b. Na 2 SO 4 ( a q ) + CaI 2 ( a q ) → CaSO 4 ( s ) + 2 NaI ( a q ) c. 2 HC 2 H 3 O 2 ( a q ) + Na 2 CO 3 ( a q ) → H 2 O ( l ) + CO 2 ( g ) + 2 NaC 2 H 3 O 2 ( a q ) d. NH 4 Cl ( a q ) + NaOH ( a q ) → H 2 O ( l ) + NH 3 ( g ) + NaCl ( a q )
Write balanced complete ionic and net ionic equations for each reaction. a. HI ( a q ) + KOH ( a q ) → H 2 O ( l ) + KI ( a q ) b. Na 2 SO 4 ( a q ) + CaI 2 ( a q ) → CaSO 4 ( s ) + 2 NaI ( a q ) c. 2 HC 2 H 3 O 2 ( a q ) + Na 2 CO 3 ( a q ) → H 2 O ( l ) + CO 2 ( g ) + 2 NaC 2 H 3 O 2 ( a q ) d. NH 4 Cl ( a q ) + NaOH ( a q ) → H 2 O ( l ) + NH 3 ( g ) + NaCl ( a q )
Solution Summary: The author explains that each chemical reaction is written in the form of complete balanced and net ionic equations.
a) A favorable entropy change occurs when ΔS is positive. Does the order of the system increase or decrease when ΔS is positive? (b) A favorable enthalpy change occurs when ΔH is negative. Does the system absorb heat or give off heat when ΔH is negative? (c) Write the relation between ΔG, ΔH, and ΔS. Use the results of parts (a) and (b) to state whether ΔG must be positive or negative for a spontaneous change. For the reaction, ΔG is 59.0 kJ/mol at 298.15 K. Find the value of K for the reaction.
A sample of hydrated magnesium sulfate (MgSO4⋅xH2O) is analyzed using thermogravimetric analysis (TGA). The sample weighs 2.50 g initially and is heated in a controlled atmosphere. As the temperature increases, the water of hydration is released in two stages: (a) The first mass loss of 0.72 g occurs at 150°C, corresponding to the loss of a certain number of water molecules. (b) The second mass loss of 0.90 g occurs at 250°C, corresponding to the loss of the remaining water molecules. The residue is identified as anhydrous magnesium sulfate (MgSO4) Questions: (i) Determine the value of x (the total number of water molecules in MgSO4⋅xH2O) (ii) Calculate the percentage of water in the original sample. Write down the applications of TGA.
The solubility product of iron(III) hydroxide (Fe(OH)3) is 6.3×10−38. If 50 mL of a 0.001 M FeCl3 solution is mixed with 50 mL of a 0.005 M NaOH solution, will Fe(OH)3 precipitate? Show all step-by-step calculations. To evaluate the equilibrium constant, we must express concentrations of solutes in mol/L, gases in bars, and omit solids, liquids, and solvents. Explain why.
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning