A student dissolves 11.3 g of sodium hydroxide (NaOH)in 300. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 22.0 °c to 31.5 °C over the course of 8.9 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 te using measured data are digits. Explanation Check Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility

A student dissolves 11.7 g of potassium hydroxide (KOH)in 200. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 23.0 °C to 33.2 °C over the course of 3.6 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: KOH(s) K+ (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 the correct number of 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 KOH.…

# H₂O(1) H*(aq) + OH(aq) Calculate the pOH of a 0.0100 M HCl solution at 50.0 °C. AH = -55.8 kJ; K=1.0 x 10-¹4 (at 25.0 °C)

NH4NO3 dissolves readily in water even though the dissolution is endothermic by 26.4 kJ/mol. Why is the process spontaneous?   Increase in enthalpy upon dissolution of this strong electrolyte. Increase in disorder upon dissolution of this strong electrolyte. The vapor pressure of the water decreases upon addition of the solute. Decrease in enthalpy upon addition of the solute.

Using the solubility rules, choose two different reactions that will yield a precipitate upon mixing. Write a procedure for determining the ΔH for these precipitation reactions.

For a certain chemical reaction, the standard Gibbs free energy of reaction at 30.0 °C is -61.4 kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 x10 S

Part b For the reaction given in Part A, how much heat is absorbed when 2.60 mol of A reacts? And part c said At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium?

If Gibbs free energy (at standard conditions) of a reaction is -22.8 kj/mol, what is the equilibrium constant of the reaction?

Calculate ArH for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and given >ArH"s Ca(s)+CO2(g)+1/202(g) →CaCO3(s), ArH= -812.8 kJmol-1 2Ca(s)+02(g) →2CaO(s), ArH= -1269.8 kJmol-1 ArH=-177.9 kJ mol-1 ArH= 177.9 kJmol-1 ArH=327.9 kJmol-1 ArH=-327.9 kJmol-1

1. Look at the attached reaction. What would you have to do to the reaction in order to increase the magnitude of K?