In the nuclear transmutation represented by Pu(He, n)?, what is the product? SHOW WITH A REACTION(S) HOW YOU ARRIVED AT YOUR ANSWER

The value of ΔG° at 373 K for the oxidation of solid elemental sulfur to gaseous sulfurdioxide is ________ kJ/mol. At 298 K, ΔH° for this reaction is -269.9 kJ/mol, and ΔS° is +11.6 J/K. SHOW WORK FOR THIS QUESTION

The more negative ΔG° is for a given reaction, the larger the value of the corresponding equilibrium constant, K. 

Which substance would be the least soluble in gasoline?

Which of the following statements are true, regarding the equilibrium constant K for a reaction and the reaction quotient Q: 1) If Q>K, the reaction is not at equilibrium and will reach equilibrium by shifting some products over to reactants. 2) If K= 3.2 x 10-6, the reaction is product favored. 3) If K = 5.2 x 104, the reaction is product favored. 4) If Q = K, the reaction is already at equilibrium.

Which of the following expressions is the correct equilibrium-constant expression for thereaction below? CO2 (s) + H2O (l) H+ (aq) + HCO3- (aq)

Which substance is the oxidizing agent in the following reaction?Fe2S3 + 12HNO3 → 2Fe(NO3)3 + 3S + 6NO2 + 6H

 BONUS #4: Based on Le Châtelier’s principle, increasing pressure at constant temperature in the following reaction will not change the concentrations of reactants and products. TELL ME HOW YOU KNOW

The beta decay of cesium-137 has a half-life of 30.0 years. How many years must pass to reduce a 25 mg sample of cesium 137 to 8.7 mg? SHOW WORK FOR THIS QUESTION

BONUS #1 Consider the reaction:FeO (s) + Fe (s) + O2(g) → Fe2O3 (s)Given the following table of thermodynamic data at 298 K: The value K for the reaction at 25 °C is ________. YOU MUST SHOW WORK FOR THIS QUESTION