O Elimination reactions are thermodynamically favored at high temperatures, where the entropy of the reaction will be larger than the enthalpy, causing a positive AG and the reactants to be favored over the products.

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

Consider the reaction CO(g) + 3H2(g)CH4(g) + H20(g) Using the standard thermodynamic data in the tables linked above, calculate G for this reaction at 298.15K if the pressure of each gas is 22.02 mm Hg. Thermodynamic Data: CO: -137.2, H2: 0, CH4: -50.7, H2O: -228.6 Consider the reaction CO(g) + 3H2(g) CH4(g) + H20(g) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if the pressure of each gas is 22.02 mm Hg. ANSWER: kJ/mol Submit Answer Retry Entire Group No more group attempts remain

2req Consider the reaction 2CO₂(g) + 5H₂(g) C₂H₂(g) + 4H₂O(g) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if the pressure of each gas is 20.84 mm Hg. ANSWER: Submit Answer Important values if needed for this question. kJ/mol Retry Entire Group 9 more group attempts remaining

Consider the reactionCO(g) + Cl2(g)COCl2(g)Using the standard thermodynamic data in the tables linked above, calculate Grxn for this reaction at 298.15K if the pressure of each gas is 37.65 mm Hg.

Q: Pure ZnO is reduced by the stoichiometric amount of carbon as in the following Reaction: ZnO (s) + C (graphite) Zn (s) + CO (g) = Heat of fusion of zinc at melting point (420°C) = 1.74 kcal/mole and heat of evaporation of zinc at boiling point (907°C) = 27.3 kcal/mole. Calculate the change in free energy for the reaction at 907 °C. Given that: Material AH°298 (kcal/mole) S° 298 C, (cal/deg/mole) (cal/deg/mole) 51+5.2x10 T- 5.7x10 T 6.8+1×10 T- 0.11×10° T ZnO(s) CO (g) C (s) Zn (s) Zn (1) & Zn (g) -83.2 10.24 - 26.42 47.14 1.48 0.71 10 5.35 + 2.4×10T 7.75

(please type answer not write by hend)

How to determine the overall ΔHo for a reaction ?

Solve 5. Investigate and analyse energy changes and rates of reactionin physical and chemical processes, and solve related problems

ch.6.8. the specific heat capacity of silver is 0.24 j/oC g a. calculate the energy required to raise the temperture of 158.0 g Ag from 271 K to 297 K b. calculate the energy required to raise the tempertyre of 1.0 mole of Ag by 1.0oC (called the molar hat capacity of silver). c. it takes 1.07kJ of energy to heat a sample of pure silver from 11.5oC to 14.8oC. calculate the mass of the sample of silver .