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Fill in the blanks
![Sign of q for the
surroundings
Sign of q for the
Part
Option
System
Surroundings
system
Zn
Water
Metal cylinders
3
в (Set 1)
CaCl,
Water
Salt
3
B (Set 2)
(NH,),CO3
Water
Salt
3
Neutralization
H,SO]
water
reaction
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- Calculating Thermodynamic Values from an Equilibrium ConstantBackgroundAs discussed in lecture, the free energy for a reaction can be related to the equilibriumconstant through the formula below.K = e (-ΔG° / RT)Therefore if Kc for a reaction is known, Go can be determined, or vice versa. Furthermore, ifyou have the value for Go at two different temperatures, you can calculate H and S throughthe familiar equation for Gibbs energy below, since you have two unknowns but also twoequations.G = H – T SIn this lab you will be studying the solubility of borax (Na2B4O5(OH)4*8H2O), a slightly solublesodium salt, at two different temperatures. When solid borax is added to water, theequilibrium below is established.Na2B4O5(OH)4*8H2O (s) 2 Na+ (aq) + B4O5(OH)42- (aq) + 8 H2O(l)If you measure the concentrations for those substances that show up in the reaction quotient,then the Kc for the reaction at that temperature can be calculated. In this lab, theconcentration of borate ion…Assuming that a bird species living in hot climates has a mass of 45 grams, calculate theminimum glucose mass required to fly to a hill 125 meters above sea level? (The amount ofchange in Gibbs energy corresponding to the oxidation of 1.0 mol of Glucose (liquid) molecule tocarbon dioxide gas and water at 25 ° C is -2808 kJ.)Calculate the change in Gibbs energy for each of the sets of ΔrH∘, ΔrS∘, and T. predict wether or not it will be spontaneous at the temprature indicated
- A system goes from state 1 to state 2 and back to state 1. (a) Is ∆E the same in magnitude for both the forward and reverse processes?For the ideal gas that proves the polytropic process with constant temperature, pressure and volume, how n = zero, 1 and infinity ?!During the industrial synthesis of methanol (CH3OH), carbon monoxide (CO) reactswith hydrogen gas. For methanol, ΔH= -100.4 kJ/mol. a) Is it preferable to maintain this system at high or low pressure? Explain.
- The boiling point of water at p = 1.0 atm is 100°C and its enthalpy of vaporization is delta Hvap = 40.7 kJ mol-1. Calculateq, w and delta Uand delta S for the process in which 2.0mol of water is vaporized at 100°C and p=1.0atmEstimate reaction enthalpy and predict the sign of reaction entropy included attatchemnt of mecahnism and of original reactionGive answer to all parts? For the system CH3COOH+ answer the following questions ?
- The molar enthalpy of fusion of ice at 273.15 K and one atm is ΔfusHm (H2O)=6.01 kJ mol-1, andthe molar entropy of fusion under the same conditions is ΔfusSm (H2O)=22.0 J K-1 mol-1. Show that(a) ΔfusGm (H2O)=0 at 273.15 K and one atm, (b) ΔfusG,m (H2O) < 0 when the temperature is greaterthan 273.15 K, and (c) ΔfusGm (H2O) > 0 when the temperature is less than 273.15 K.If 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?The ∆G° of vaporization for butane at 298 K and 1.00 atm is -2.125 kJ/mol. Calculate the pressure of butane vapor in equilibrium with butane liquid at 298 K.