Consider the reaction for the dissolution of borax in water. Does the reaction shift to the right or to the left as temperature increases (i.e., as the reaction is stressed by the application of increased temperature/additional heat)? Based on this shift, do you expect the dissolution of borax in water to be exothermic or endothermic?

Given the following: P,(s) + 50,(g) → P,0,(s) A G° = – 2697.0 kJ/mol2H, (g) +0,(g) → 2H,0(g) A G° = – 457.18 kJ/mol 6H,0(g) +P_0 10(s) →4H,PO¸(1) AG° = - 428.66 kJ/mol What is the standard free energy of formation, A Gf°, for phosphoric acid? (A) 11243.3 kJ/mol (B) -4497.2 kJ/mol c) 4497.2 kJ/mol D -11243.3 kJ/mol

If AH = -73.54 kJ for a chemical reaction, that reaction O Endothermic O Spontaneous Exothermic O Exergonic

What is the change in the energy of surroundings when the system absorbs 17.5 kJ of energy and performs 5.00 x 10^3 J of work on the surroundings? a. +22.5kJ b. +17.5 kJ c. –22.5 kJ d. +12.5kJ e. –12.5 kJ

The reaction 4AI (s) + 30 2 (g) → 2 Al 20 3 (s)AH° = -3351 kJ is and therefore heat is by the reaction. A) thermoneutral, neither released nor absorbed B exothermic, released (C) endothermic, released D) exothermic, absorbed E) endothermic, absorbed

Propylene glycol (C3H8O2) is an important compound used to de-ice airplanes before take-off and as RV antifreeze due to it being relatively non-toxic. A plausible reaction for the production of ethylene glycol is:  2 CO (g) + 2 H2 (g) + CH4 (g) -> C3H8O2 (l)  Using the thermodynamic properties from the following table, what is the value for ΔrS°, in units of J K-1‑mol-1 at 25 °C? Substance  ΔfH° (kJ/mol)  S° (J/Kmol)  CO (g)  -110.5  197.7  H2 (g)  0  130.7  CH4 (g)  -74.6  186.3  C3H8O2 (l)  -429.8  93.7

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)

Measurements show that the enthalpy of a mixture of gaseous reactants increases by 238. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 197. kJ of work is done on the mixture during the reaction 1. Calculate the change in energy of the gas mixture during the reaction. Round your answer to 3 significant digits.2. Is the reaction exothermic or endothermic?

calculate delta G (kJ/mol) for the following reaction at 298 K when P_H2=0.0200 atm and P_C3H8=0.500 atm  3C(s, graphite)+4H2(g)=>C3H8(g)

What is the relationship between the two? Which is more stable in terms of thermodynamics, why?