Determine if the indicated experimental change (on left) would cause an increase, decrease or no change to the solubility of a salt whose AHsolution = +15 kJ mol"1 adding heat A increase solubility surrounding the solution and the beaker with an ice bath B. decrease solubility Cno change to solubility
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- Calculate the Enthalpy of change in Kj/mol and % difference in the neutralization reaction below: HNO2 + NH3 = N2 + 2 H2O Initial Temp= 20 Deg celsius Final Temp= 22.3 Deg celsius Conc= 0.4 M [HNO3] and 0.4 M [NH3] Vol= 55 mL [HNO2] and 60 mL [NH3]= Mass is 115 g Specific Heat= 4.184 J/g For the other value in % difference use: -348 Kj/molHow does the heat or enthalpy of the reaction (ΔHrxn) change when the concentration of a Strong acid (HCl) is increasing and the concentration of strong base (NaOH) is kept constant in a solution mixture? plz answer showing the steps to solve quantatiavely using hess's law. ive also attached images of my lab data for referenceFor the reaction: CuS (s) + H₂(g) → H₂S (g) + Cu (s) Given: ΔS ⁰ (CuS) = 66.5 J/mole-K ΔHf ⁰ (CuS) = -53.1 kJ/mol ΔS ⁰ (H₂S) = 205 J/ mole-K ΔHf ⁰ (H₂S) = -20.6 kJ/mol ΔS ⁰ (Cu) = 33.3 J/ mole-K ΔH f ⁰ (Cu) = 0.0 kJ/mol ΔS ⁰ (H₂) = 131 J/ mole-K ΔH f ⁰(H₂) = 0.0 kJ/mol The standard free energy of the reaction ΔG ⁰ rxn is A) -37.9 kJ/mole B) 44.6 kJ/mole C) -20.3 kJ/mole D) +20.3kJ/mole and spontaneous E) +37.9 kJ/mole
- Calcium hydroxide is a base that does not dissolve very well in water. When saturated, a calcium hydroxide solution at 25°C contains 1,3 gram Ca(OH)2 per dm3 solution. The molar mass of Ca(OH)2 is 74,1 g×mol–1. When the Ca(OH)2 dissolves, the following reaction represents the solubility equilibrium: Ca(OH)2 (s) D Ca2+ (aq) + 2 OH– (aq) Use this information above to find the value of Ksp for Ca(OH)2 at 25°C.The solubility of ZnS(s) in water at a certain temperature is 1.4 × 10–11 mol/L, i.e., x or the [Zn+2]=[S-2]. The value of the Ksp of ZnS isA 5.00 g sample of an unknown salt is dissolved in 50.0 mL of water. During dissolution, the temperature of the solution increases from 24.53 oC to 26.82 oC. Which statement(s) is(are) true? qsurroundings > 0 qsystem < 0 qsystem > 0 qsurroundings < 0 (You can choose more than one)
- The solubility of Cd(OH)2 in water at a certain temperature is 2.0 × 10–5 mol/L, (i.e., x). The Ksp value for Cd(OH)2 isThe molar solubility of rhombic sulfur (S(s, rhombic)) in water is very slight, only 1.9x10-8 mol/L. Compute for the dissolution of rhombic sulfur in water a. 44.1 kJ/mol b. 3.7 kJ/mol c. 19.1 kJ/mol d. -19.1 kJ/mol e. additional date is requiredIf qrxn =-2000 J, the equation has 1:1 mole ratio, and their are 0.00125 moles of limiting reagent. What is deltaH, when deltaH = q/n?
- Given: MnS + H+ < -- > Mn2+ + HS- CuS + H+ < -- > Cu2+ + HS- [A] Classify each reaction as exothermic or endothermic based on the DGr0 (Gibbs energy in kJ/mol). [B] What is the Ksp of MnS and CuS? [C] Which is more soluble? Gibbs free energy given in kJ/mol: CuS = −86.2 MnS = 30In lecture I mentioned that standard state is usually at 25oC; however, it can be at any specified temperature. In problems 9 and 10 you will calculate ΔGo from Ksp data. The Ksp range over the temperature range in these two problems is consistent with some actual solubility data; however, in order to allow each student to do their own calculation I have made this data for an "unknown" ionic solid. Calculate the value of ΔGo (kJ/mol) at 3.3oC for the dissolution of an ionic solid with a Ksp of 2.5 x 10-11 at 3.3oC. Your answer should have 2 sig figs.A 51.0-LL reactor at 1600 KK is charged with 50.0 gg of NiO(s)NiO(s) and 1.40 atmatm of CO(g)CO(g). After equilibrium is reached, what is the partial pressure of CO2(g)CO2(g) in the reactor?