For a hypothetical reaction, ΔrHθ = 89.1 kJ/mol and ΔrSθ = 364 J/mol/K. What is the...

For a hypothetical reaction, ΔrHθ = 89.1 kJ/mol and ΔrSθ = 364 J/mol/K. What is the total standard entropy of the reaction, ΔrStotθ, at 343 K?

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

A reaction has and △H°298 = 151 kJ/mol and △S°298 = 286 J /mol K at...

A reaction has and △H°298 = 151 kJ/mol and △S°298 = 286 J /mol K at 298 K. Calculate △G in kJ/mol.

Cgas = 1.3 J/g×K Hvap = 38.56 kJ/mol Cliq = 2.3 J/g×K Hfus = 5.02 kJ/mol ...

Cgas = 1.3 J/g×K Hvap = 38.56 kJ/mol Cliq = 2.3 J/g×K Hfus = 5.02 kJ/mol Csolid = 0.97 J/g×K Condensation Temp = 78.0oC Freezing Pt = -114.0oC Calculate the amount of heat required toconvert 92.6 mL of ethanol, C2H6O, from 110.0oC to -98.0oC.

Estimate Keq for the following equilibria at 350 K. R = 8.3145 J/(molK). Substance ΔHo(kJ/mol) So(J/(molK))...

Estimate Keq for the following equilibria at 350 K. R = 8.3145 J/(mol*K). Substance ΔHo(kJ/mol) So(J/(mol*K)) SnO2(s) -577.6 49.0 H2(g) 0 130.680 CO(g) -110.5 197.7 Sn(s, white) 0 51.2 H2O(l) -285.83 69.95 Fe(s) 0 27.3 Fe3O4(s) -1118.4 146.4 Correct answer. Correct. SnO2(s) + 2H2(g) ⇄ Sn(s, white) + 2H2O(l) The number of significant digits is set to 2; the tolerance is +/-3% LINK TO TEXT Incorrect answer. Incorrect. 3Fe(s) + 4H2O(l) ⇄ Fe3O4(s) + 4H2(g) Entry field with incorrect answer...

Suppose Delta G^o is 25.0 KJ/mol for a hypothetical reaction in which A converts into B....

Suppose Delta G^o is 25.0 KJ/mol for a hypothetical reaction in which A converts into B. Which of the following statements describes an equlibrium mixture of A and B? a) B has a higher concentration than A. b) Only A is present. c) A and B have equal concentrations. d) Only B is present. e) A has a higher concentration than B. Could you please explain your reasoning behind the answer as well?

For the reaction below, Δ S ° = − 269 J/(mol · K) and Δ H...

For the reaction below, Δ S ° = − 269 J/(mol · K) and Δ H ° = − 103.8 kJ/mol. Calculate the equilibrium constant at 25 °C. 3C(s) + 4H_2 (g) -->C_3+ H_8 (g)

For a particular reaction at 129.9 °C, ΔG = 319.61 kJ/mol, and ΔS = 777.00 J/(mol·K)....

For a particular reaction at 129.9 °C, ΔG = 319.61 kJ/mol, and ΔS = 777.00 J/(mol·K). delta g is -47.6 celcius

For a particular reaction at 234.1 °C, ΔG = -832.94 kJ/mol, and ΔS = 923.32 J/(mol·K)....

For a particular reaction at 234.1 °C, ΔG = -832.94 kJ/mol, and ΔS = 923.32 J/(mol·K). Calculate ΔG for this reaction at -105.7 °C.

For a particular reaction at 215.7 °C, ΔG = 404.91 kJ/mol, and ΔS = 748.20 J/(mol·K)....

For a particular reaction at 215.7 °C, ΔG = 404.91 kJ/mol, and ΔS = 748.20 J/(mol·K). Calculate delta G for -74.3 celcius. I've asked this question previously and the individual who answered got roughly 378 kj/mol which is incorrect.

The reaction C4H8(g)⟶2C2H4(g)C4H8(g)⟶2C2H4(g) has an activation energy of 262 kJ/mol.262 kJ/mol. At 600.0 K,600.0 K, the...

The reaction C4H8(g)⟶2C2H4(g)C4H8(g)⟶2C2H4(g) has an activation energy of 262 kJ/mol.262 kJ/mol. At 600.0 K,600.0 K, the rate constant, ?,k, is 6.1×10−8 s−1.6.1×10−8 s−1. What is the value of the rate constant at 765.0 K?

Consider a reaction with the following thermodynamic properties. ΔH° = 77.7 kJ ΔS° = –35.7 J/(K...

Consider a reaction with the following thermodynamic properties. ΔH° = 77.7 kJ ΔS° = –35.7 J/(K • mol) ΔG°= 88.4 kJ This reaction: will proceed very slowly. will be spontaneous at low temperatures. has bonds in the products that are weaker than the reactants. may have fewer and more complicated molecules in the product.

Subjects