Calculate the masses of (a) Ca(NO3)2 and, separately, (b) NaCI to add to a 0.150 mol kg-1 solution of KNO3(aq) containing 500 g of solvent to raise its ionic strength to 0.250.
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Calculate the masses of (a) Ca(NO3)2 and, separately, (b) NaCI to add to a 0.150 mol kg-1 solution of KNO3(aq) containing 500 g of solvent to raise its ionic strength to 0.250.
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- Calculate the masses of (i) KNO3 and, separately, (ii) Ba(NO3)2 to add to a 0.110 mol kg−1 solution of KNO (aq) containing 500 g of solvent to raise its ionic strength to 1.00.The standard Gibbs energy of formation of rhombic sulfur is zero and that of monoclinic sulfur is +0.33 kJ mol-1, at 25 °c.Which polymorph is the more stable at that temperature?Calculate the standard Gibbs energy of reaction for 4 HI(g) + O2(g) → 2 I2(s) + 2 H2O(l) at 298 K, using the values of standard entropies and enthalpies of formation given in the Resource section.
- The standard Gibbs energy of the reaction 2 NO2(g) → N2O4(g) is −4.73 kJ mol−1 at 298 K. What is the value of ΔrG when Q = (i) 0.10, (ii) 1.0, (iii) 10, (iv) 100? Estimate (by interpolation) the value of K from the values you calculate. What is the actual value of K?The excess Gibbs energy of a certain binary mixture is equal to gRTx(1 − x) where g is a constant and x is the mole fraction of a solute B. Find an expression for the chemical potential of B in the mixture and sketch its dependence on the composition.By how much does the chemical potential of carbon dioxide at 310 K and 2.0 bar differ from its standard value at that temperature?
- Certain bacteria in the soil obtain the necessary energy for growth by oxidizing nitrite to r nitrate: 2NO2- (aq) + O2(g) —> 2NO3-(aq) Given that the standard Gibbs energies of formation of NO2- and NO3- are -34.6 kJ mol-1 and -110.5 kJ mol-1, respectively, calculate the amount of Gibbs energy released when 1 mole of No2- is oxidized to 1 mole of NO3-.The molar conductivity of 0.010 M CH3COOH(aq) is 1.65 mS m2 mol-1. What is the acidity constant, Ka, of the acid?The standard enthalpy of combustion of the solid glycine (the amino acid, NH2CH2COOH) is −969 kJ mol−1 at 298 K and its standard molar entropy is 103.5 J K−1 mol−1. Calculate the standard Gibbs energy of formation of glycine at 298 K. Note that the nitrogen-containing species produced on combustion is taken to be N2(g).
- The standard Gibbs energy of formation of PH3(g) is +13.4 kJ mol−1 at 298 K. What is the corresponding reaction Gibbs energy when the partial pressures of the H2 and PH3 (treated as perfect gases) are 1.0 bar and 0.60 bar, respectively? What is the spontaneous direction of the reaction in this case?One of the most extensively studied reactions of industrial chemistry is the synthesis of ammonia, for its successful operation helps to govern the efficiency of the entire economy. The standard Gibbs energy of formation of NH3(g) is -16.5 kJ mol-1, at 298 K. What is the reaction Gibbs energywhen the partial pressure of the N2, H2, and NH3 (treated as perfect gases) are 3.0 bar, 1.0 bar, and 4.0 bar, respectively?What is the spontaneous direction of the reaction in this case?The standard enthalpy of combustion of liquid ethyl ethanoate (ethyl acetate, CH3COOC2H5) is −2231 kJ mol−1 at 298 K and its standard molar entropy is 259.4 J K−1 mol−1. Calculate the standard Gibbs energy of formation of the compound at 298 K.