When sodium chloride dissolves in water, the ions dissociate: NaCl (s) Na+ (aq) + Cl- (aq)
What is the sign of the change in Gibbs free energy (DG) for each process in the forward direction?
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When sodium chloride dissolves in water, the ions dissociate: NaCl (s) Na+ (aq) + Cl-...
When sodium chloride dissolves in water, the ions dissociate: NaCl (s) --> Na+ (aq) + Cl- (aq) Consider the equation, DG = DH - TDS. For each dissolving process, substitute the signs of DG and DH into the equation and predict the possible sign(s) for the entropy (DS). Explain why you chose this sign(s). Does the sign for entropy change seem to make sense? Explain.
When sodium chloride dissolves in water, the ions dissociate: NaCl (s) à Na+ (aq) + Cl- (aq) Write ionic equations, similar to the one above, that describe how NaNO3 and NaCH3COO each dissociate as they dissolve in water. Include heat as a reactant or product in each equation
When sodium chloride dissolves in water, the ions dissociate: NaCl (s) --> Na+ (aq) + Cl- (aq) Write ionic equations, similar to the one above, that describe how NaNO3 and NaCH3COO each dissociate as they dissolve in water. Include heat as a reactant or product in each equation.
10. When sodium chloride dissolves in water, the ions dissociate: NaCl (s) = Na+ (aq) + Cl- (aq) Write ionic equations, similar to the one above, that describe how NaNO3 and NaCH3CO2 each dissociate as they dissolve in water. Include heat as a reactant or product in each equation. Here is what I answered: NaNO3 (s) = Na+ + NO3- + heat NaC2H3O2 + Heat = Na+ + C2H3O2-(ag) Lab data table attached to determine where to place heat. AGO no...
I need help with 11 and 12 please. Data Table Mixture NaCl (s) + H2O (1) T (initial) T, (final) AT (T-T) -.20 25.00 24.80 NaNO, (s) + H2O (1) 24.99 24.11 -.88 NaCH,COO + H2O (1) 24.99 25.91 .82 Use your experimental data to answer the following questions: 7. Calculate AT (AT = T2-T) for each mixture and record the results in the data table. 8. An exothermic process releases heat (warms up), and an endothermic process absorbs heat...
Sodium (Na) atoms are larger than chlorine (Cl) atoms, but in NaCl sodium ions (Na+) are much smaller than chloride (Cl-) ions. Discuss why there is a change in size of each element (i.e., why is Na --> Na+ a decrease in size and Cl --> Cl- is an increase in size).
The following enthalpy change is known for the dissolution of sodium chloride in water. What is the energy needed or released for the dissolution of 58.44g of sodium chloride in water? NaCl (s) Na* (aq) + Cl- (aq) AH = +3.87 kJmol-1
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(s)ΔH=−65.5kJ Calculate ΔH for formation of 0.490 mol of AgCl by this reaction. Calculate ΔH for the formation of 7.50 g of AgCl. Calculate ΔH when 9.23×10−4 mol of AgCl dissolves in water.
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(s)ΔH=−65.5kJ A.) Calculate ΔH for formation of 0.100 mol of AgCl by this reaction. I got A ΔH=-6.55 kJ B.) Calculate ΔH for the formation of 2.80 g of AgCl. C.) Calculate ΔH when 0.110 mmol of AgCl dissolves in water. Need help with B and C.
11. Insoluble silver chloride dissolves in the presence of chloride ion. The equation for the overall reaction is AgCl(s) + Cl(aq) AgCl2 (aq) a) show that the overall reaction is the sum of two others: the ionization of AgCl(s) to give silver(I) and chloride ions, and the formation of AgCl2 (aq) from Ag (aq) and Cl(aq) ions. b) Calculate the equilibrium constant for the overall process from the equilibrium constants for the two steps. (refer back to Complex lon Formation...