A key step in the production of sulfuric acid is the oxidation of SO2(g) to SO3(g):                         2SO2(g) + O2(g) → 2SO3(g)At 298 K, ΔG = 2141.6 kJ; ΔH = 2198.4 kJ; and ΔS = 2187.9 J/K.(a) Use the data to decide if this reaction is spontaneous at 25°C, and predict how ΔG will change with increasing T.(b) Assuming that ΔH and ΔS are constant with T (no phase change occurs), is the reaction spontaneous at 900.°C?

The decomposition of N,0, can be described by the equation 2 N,0,(soln) → 4NO, (soln) + O,(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. 1 (s) [N,O3] (M) 2.576 215 2.250 456 1.934 755 1.602 Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time interval from 0 s to 215 s? average rate of reaction: M/s What is the average rate of reaction for the time interval from 215 s to 456 s? average rate of reaction: M/s What is the average rate of reaction for the time interval from 456 s to 755 s? average rate of reaction: M/s

A change in a system occurs such that 40.6 J of heat flows in to the system and 48.0 J of work is done by the system. What is the change in internal energy of the system? O a.-7.4 J O b. -88.6 J O c. 7.4 J O d. 88.6 J O e. -48.0 J

A student determines the value of the equilibrium constant to be 1.98×10-5 for the following reaction.CO2(g) + H2(g)CO(g) + H2O(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank 1 than zero.Calculate the free energy change for the reaction of 1.74 moles of CO2(g) at standard conditions at 298K.     G°rxn =  kJ