For a certain chemical reaction, the standard Gibbs free energy of reaction is  129.   kJ . Calculate the temperature at which the equilibrium constant K   =   ×6.010−25 . Round your answer to the nearest degree.

For a certain chemical reaction, the standard Gibbs free energy of reaction is 83.7 kJ. Calculate the temperature at which the equilibrium constant K = 1.9x 10-16 Round your answer to the nearest degree.

A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction ATP(aq) + H,O(1) → ADP(aq) + HPO (aq) for which AGxn = –30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of AGrn in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.30 mM, and [HPO,] = 5.0 mM. AGxn = kJ/mol TOOLS x10 Is the hydrolysis of ATP spontaneous under these conditions? yes no Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publisher: University Science Books

A well insulated calorimeter containing 100 ml of water was calibrated by dissolving. known amount of potassium chloride in the calorimeter. The dissolution of potassium chloride in water can be represented by the equation: KC(s) + aq- AH = +17.0 kJ mol K*(aq) + Cl(aq) The temperature of the calorimeter was initially 18.00 °C. A sample of 2.46 g of potassium chloride was dissolved in the 100 ml and the temperature was recorded as 16.60 °C. The calibration factor of the calorimeter is (express your answer to 2 decimal places) 0.40 kJ *C¹

1. When 2.35g Mg(OH)₂ is added to 250.0 mL of water, the temperature of the water raises from 20.5°C to 36.0°C. Calculate the molar enthalpy of solution.

Calculate the standard enthalpy change for the reaction at 25 ∘25⁢ ∘C. Standard enthalpy of formation values can be found in this list of thermodynamic properties.   Mg(OH)2(s)+2HCl(g)⟶MgCl2(s)+2H2O(g)

Calculate the standard change in Gibbs free energy, Δ?∘rxnΔ⁢Grxn∘ , for the given reaction at 25.0 ∘C25.0⁢ ∘C . Consult the table of thermodynamic properties for standard Gibbs free energy of formation values.   NH4Cl(s)↽−−⇀NH+4(aq)+Cl−(aq)

A student observed that, when 0.243 g of magnesium was added to 100.0 g of hydrochloric acid, the temperature of the solution increased 11.2 °C. Without doing any calculations, what observations can you make to support your claim that the reaction that occurred between magnesium and hydrochloric acid was exothermic?

A student dissolves 11.4 g of sodium hydroxide (NaOH)in 200. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 20.0 °C to 35.7 °C over the course of 3.7 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH (s) Na(aq) + OH (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 3 significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔΗ per mole of NaOH. rxn exothermic…

For a certain chemical reaction, the equilibrium constant K = 4.5 × 10 - 10 at 5.00 °C. Calculate the standard Gibbs free energy of reaction. %3D Round your answer to 2 significant digits. AG° = | kJ |x10