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The magnitude of ΔHrxn of HNO3 will _____________ when a chemist uses a wet pipette in transferring the sample.
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- Is each of the following permissible? Explain. If not, provide a permissible combinationa) (4, -1, 0, -1/2)b) (3, 2, -3, +1/2)81.6 g of a metal alloy was heated to 93 o C, then plunged into 105 mL of H 2O that was at 19.5 o C. The system equilibrated at 22.3 oC. What is the specific heat of the metal?What is the change in enthalpy in joules when 10.5g of AgCl (143.3g/mol) dissolves in water according to the following chemical equation: AgCl(s) à Ag+(aq) + Cl-(aq) ΔH°rxn = 65.5 kJ/mol
- Develop a general equation for the standard heat of reaction as a function of temperature for one of the reactions given in parts a, b, c a. N2(g)+3H2(g) → 2NH3(g) b. 4NH3(g) +5O2(g) → 4NO(g)+6H2O(g) c. 2Na(s)+2H2O(g) →2NaOH(s)+H2(g)Develop a general equation for the standard heat of reaction as a function of temperature for one of the reactions given in parts (a), (b), (c) a. H2S(g) + 2H2O(g) → 3H2(g) + SO2(g) b. N2(g) + O2(g) → 2NO(g) c. CaCO3(s) → CaO(s) + CO2 (g)What is the entropy at SATP of a reaction where ∆Hºrxn=12.5 kJ and Keq=32.1?
- Calculate ΔH°298 for the processSb(s) + (5)/(2)Cl2(g) ⟶ SbCl5(g)from the following information:Sb(s) + (3)/(2)Cl2(g)⟶SbCl3(g) ΔH°298 = −314 kJSbCl3(s) + Cl2(g)⟶SbCl5(g) ΔH°298 = −80 kJQ26-C (i) Explain pyrolysis process.Develop a general equation for the standard heat of reaction as a function of temperature for one of the reactions given in parts (a), (b), (c) a. CO2(g) + 3H2(g) → CH3OH(g) + H2O(g) b. CH3OH(g) + 1/2O2(g) → HCHO(g) + H2O(g) c. 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g)
- An aqueous solution of cobalt(II) chloride, CoCl2, is made by dissolving 2.07 grams of cobalt(II) chloride in sufficient water in a 50.0 mL volumetric flask, and then adding enough water to fill the flask to the mark. What is the weight/volume percentage of cobalt(II) chloride in the solution? Weight/volume percentage = ______% How many grams of iron(III) fluoride, FeF3, are required to make a 6.28 %(w/v) aqueous solution in a 300. mL volumetric flask? ________gDevelop a general equation for the standard heat of reaction as a function of temperature for one of the reactions given in parts (a), (b) a. CO2 (g) + 3H2 (g) → CH3OH(g) + H2O(g) b. C2H2 (g) + H2O(g) → ⟨(CH2)2⟩O(g)A coffee cup calorimeter with a heat capacity of 4.90 J/∘C was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL solution of 0.360 M AgNO3 was mixed with 50.0 mL of 0.480 M KCl. After mixing, the temperature was observed to increase by 2.80∘C.Calculate the enthalpy of reaction, Δ?rxn, per mole of precipitate formed (AgCl). Assume the specific heat of the product solution is 4.17 J / (g⋅∘C) and that the density of both the reactant solutions is 1.00 g/mL. Calculate the theoretical moles of precipitate formed from AgNO3 and KCl. Calculate the heat change experienced by the calorimeter contents, ?contents. Calculate the heat change experienced by the calorimeter, ?cal. Calculate the heat change produced by the solution process, ?solution. Calulate Δ?solution for one mole of precipitate formed. I'm just going to go ahead and say thank you to whoever decides to answer this question. I really appreciate the help I have received. ?