In the environment, the equilibrium between calcite and dissolved calcium and carbonate is defined by this reaction: CaCO3 (s) ⇌ Ca2+ + CO3 2- .
The answer to the question above could be obtained by comparing the reaction quotient Q (based on a specific solution composition) to the thermodynamic constant K.
a. Calculate the thermodynamic constant K from on the standard Gibb free energy of reaction ΔGº r.
b. A water sample contains 0.22 mmol Ca kg-1 and 0.05 mmol CO3 2- kg-1 . Calculate the reaction quotient Q.
c. Compare the values of Q and K obtained to answer to the question above.
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In the environment, the equilibrium between calcite and dissolved calcium and carbonate is defined by this...
Problem 5.28. Calcium carbonate, CaCO3, has two common crystae forms, calcite and aragonite. Thermodynamic data for these phases can be found at the back of this book (a) Which is stable at earth...
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3) The dissociation of ammonium nitrate in aqueous solutions is described by the following chemical reaction...
3) The dissociation of ammonium nitrate in aqueous solutions is described by the following chemical reaction Use the information provided in the table below at 25°C, to plot the Gibbs free energy change as a function of the natural logarithm of Q, InQ. [Recall that Q is the quotient of the product of the products raised to the stoichiometric coefficients over the product of the reactants raised to their stoichiometric coefficients.] a) On the ΔG vs In(Q) plot indicate the...
A student determines the value of the equilibrium constant to be 1.5297 x 107 for the...
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Calculate the change in Gibbs free energy at standard conditions (TSS) and the equilibrium constant for...
Calculate the change in Gibbs free energy at standard conditions (TSS) and the equilibrium constant for each of the following reactions. (a) CH4(g) + H2O(g) equilibrium reaction arrow CO(g) + 3 H2(g); ?H° = +205.9 kJ, ?S° = +214.7 J/K ?G° 141.9 Correct: Your answer is correct. kJ K (b) CaCO3(s) equilibrium reaction arrow CaO(s) + CO2(g); ?H° = +179.2 kJ, ?S° = +160.2 J/K ?G° 131.5 Correct: Your answer is correct. kJ K
Calculate the free energy AG at 25°C for the nonstandard conditions at point where the reaction...
Calculate the free energy AG at 25°C for the nonstandard conditions at point where the reaction quotient Q is 2.75 x 10 Express your answer numerically in kilojoules. View Available Hint(s) % ALC O ? AG - CO Nitrosyl chloride formation Chlorine gas. Cl(s), reacts with nitric oxide, NO(), to form nitrosyl chloride, NOCI(g), via the reaction Cl(s) + 2NO(g) + 2NOCI() The thermodynamic data for the reactants and products in the reaction are given in the following table: Substance...
The condition of a system at equilibrium represents a balance between the tendency toward lowest energy...
The condition of a system at equilibrium represents a
balance between the tendency toward lowest energy (E) and
the tendency toward molecular chaos or maximum entropy (S). The
Gibbs Free Energy, G, is the state function that combines energy
and entropy into an equation that allows us to find the balance
between these two tendencies. For a system undergoing change at
constant temperature, ΔG = ΔH - TΔS. The system stops changing when
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AGO/kJ mol -109.7 378.5 -10.8 - 1576.4 0.0 3.1 -604.2 -1128.8 0.0 2.9 Compound AgCl(s) AgN,(s) Ag,O(s) Al2O3(s) Bre(2) Bre(g) | Cabs) CaCO,(s) C-graphite C-diamond CH (g) CH2(g) C.H.(g) C2H6g) CeHel) CO(g) CO2(g) CuO (8) Fe2O3(s) HBr(g) HCl(g) HI(g) -50.8 209.2 68.2 -32.9 124.5 -137.3 -394.4 -127.2 -741.0 -53.2 -95.3 Compound H2O(g) H2O(1) H2O2(1) H,S(g) HgO(s) Iz(s) Iz(g) KCl(s) KBr(s) MgO(s) MgH (s) NH3(g) NO(g) NO2(g) N20 (g) NF (g) NaCl(s) NaBr(s) Os(g) SO2(g) SO2(g) ZnO(s) AGO/kJ mol -228.6 -237.2...
Task 2. Using standard values of free energy AG, determine AG for the following ion-exchange reac...
Task 2. Using standard values of free energy AG, determine AG for the following ion-exchange reactions and draw a conclusion about their possible direction. Examine results experimentally Caco, + 2H+-> H2O + Ca + CO2 To determine neutralization heat AHacestr it is necessary to refer the heat quantity to 1 mole of the substance, namely to alkali since acid is taken in excess (see alkalis and acids molarities and volumes). It is also necessary to take into account that ΔΗ...
The equilibrium constant of a system, K, can be related to the standard free energy change,...
The equilibrium constant of a system, K, can be related to the standard free energy change, ΔG∘ ΔG∘=−RTlnK where T is a specified temperature in kelvins (usually 298 KK) and R is equal to 8.314 J/(K⋅mol) Under conditions other than standard state, the following equation applies: ΔG=ΔG∘+RTlnQ In this equation, Q is the reaction quotient and is defined the same manner as KK except that the concentrations or pressures used are not necessarily the equilibrium values. Part A Acetylene, C2H2,...
help with this please Ca(OH)2(aq) + 2 HCl(aq) +CaCl2(8) + 2 H2O(1) Using the standard thermodynamic...
help with this please
Ca(OH)2(aq) + 2 HCl(aq) +CaCl2(8) + 2 H2O(1) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: N2(g) + O2(g) +2NO(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: 2CO(g) + O2(g) +2002(9) - der e en manos de 20, ali ne more than one so mi dicogna undan Using standard thermodynamic data...
Problem 5.28. Calcium carbonate, CaCO3, has two common crystae forms, calcite and aragonite. Thermodynamic data for these phases can be found at the back of this book (a) Which is stable at earth's surface, calcite or aragonite? (b) Calculate the pressure (still at room temperature) at which the other phase should become stable. All of the values in this table are for one mole of material at 298 K and 1 bar. Following the chemical formula is the form of...
3) The dissociation of ammonium nitrate in aqueous solutions is described by the following chemical reaction Use the information provided in the table below at 25°C, to plot the Gibbs free energy change as a function of the natural logarithm of Q, InQ. [Recall that Q is the quotient of the product of the products raised to the stoichiometric coefficients over the product of the reactants raised to their stoichiometric coefficients.] a) On the ΔG vs In(Q) plot indicate the...
Calculate the free energy AG at 25°C for the nonstandard conditions at point where the reaction quotient Q is 2.75 x 10 Express your answer numerically in kilojoules. View Available Hint(s) % ALC O ? AG - CO Nitrosyl chloride formation Chlorine gas. Cl(s), reacts with nitric oxide, NO(), to form nitrosyl chloride, NOCI(g), via the reaction Cl(s) + 2NO(g) + 2NOCI() The thermodynamic data for the reactants and products in the reaction are given in the following table: Substance...
The condition of a system at equilibrium represents a
balance between the tendency toward lowest energy (E) and
the tendency toward molecular chaos or maximum entropy (S). The
Gibbs Free Energy, G, is the state function that combines energy
and entropy into an equation that allows us to find the balance
between these two tendencies. For a system undergoing change at
constant temperature, ΔG = ΔH - TΔS. The system stops changing when
it reaches the equilibrium condition, ΔG =...
AGO/kJ mol -109.7 378.5 -10.8 - 1576.4 0.0 3.1 -604.2 -1128.8 0.0 2.9 Compound AgCl(s) AgN,(s) Ag,O(s) Al2O3(s) Bre(2) Bre(g) | Cabs) CaCO,(s) C-graphite C-diamond CH (g) CH2(g) C.H.(g) C2H6g) CeHel) CO(g) CO2(g) CuO (8) Fe2O3(s) HBr(g) HCl(g) HI(g) -50.8 209.2 68.2 -32.9 124.5 -137.3 -394.4 -127.2 -741.0 -53.2 -95.3 Compound H2O(g) H2O(1) H2O2(1) H,S(g) HgO(s) Iz(s) Iz(g) KCl(s) KBr(s) MgO(s) MgH (s) NH3(g) NO(g) NO2(g) N20 (g) NF (g) NaCl(s) NaBr(s) Os(g) SO2(g) SO2(g) ZnO(s) AGO/kJ mol -228.6 -237.2...
Task 2. Using standard values of free energy AG, determine AG for the following ion-exchange reactions and draw a conclusion about their possible direction. Examine results experimentally Caco, + 2H+-> H2O + Ca + CO2 To determine neutralization heat AHacestr it is necessary to refer the heat quantity to 1 mole of the substance, namely to alkali since acid is taken in excess (see alkalis and acids molarities and volumes). It is also necessary to take into account that ΔΗ...
help with this please
Ca(OH)2(aq) + 2 HCl(aq) +CaCl2(8) + 2 H2O(1) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: N2(g) + O2(g) +2NO(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: 2CO(g) + O2(g) +2002(9) - der e en manos de 20, ali ne more than one so mi dicogna undan Using standard thermodynamic data...
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