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Consider the following reaction at 298 K. C ( graphite ) + 2 H 2 ( g ) ⟶ CH 4 ( g ) Δ H ∘ = − 74.6 kJ and Δ S ∘ = − 80.8 J / K Calculate the following quantities. Δ S sys = J/K Δ S surr = J/K Δ S univ = J/K Is this reaction spontaneous? yes no
Consider the following reaction at 298 K. C ( graphite ) + 2 H 2 ( g ) ⟶ CH 4 ( g ) Δ H ∘ = − 74.6 kJ and Δ S ∘ = − 80.8 J / K Calculate the following quantities. Δ S sys = J/K Δ S surr = J/K Δ S univ = J/K Is this reaction spontaneous? yes no
Final answer:The reaction is spontaneous at 298 K as indicated by a negative ΔG. The entropy of the system decreases, signifying an increase in order, while the entropy of the surroundings increases. The total entropy change in the universe is positive.Explanation:To determine if this reaction is spontaneous, we need to calculate the Gibbs free energy change (ΔG) using the formula ΔG = ΔH - T*ΔS, where ΔH is the change in enthalpy, T is the absolute temperature in Kelvin, and ΔS is the change in entropy.First, we convert ΔH and ΔS to the same units. Here, ΔH is in kJ and ΔS is in J/K. So, we convert ΔH = -74.6 kJ to J which gives ΔH = -74600 J. Plugging these values into the equation gives ΔG = -74600J - 298K * -80.8J/K = -51216 J or -51.216 kJ.Since ΔG is negative, we can say the reaction isspontaneousat 298 K. For the system, the negative ΔS indicates order is increasing, and for the surroundings, ΔS is ΔH/T = 74600/298 = 250.67 J/K. Finally, The total entropy change in the universe ΔS univ can be calculated using ΔS univ = ΔS sys + ΔS surr and comes out to be 169.87 J/K.Learn more about Spontaneity of Reaction here:brainly.com/question/32274705#SPJ3...