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455 solutions

Gibbs Free Energy

Q. The values of Delta H and delta S for the reaction of nitrogen monoxide plus oxygen going to nitrogen dioxide are -12 KJ and -146 J/K at 298 K. Calculate Delta G.

Solved • Apr 4, 2020

Gibbs Free Energy

Q. 4. Calculate ΔG for the following reaction at 25°C. Will the reaction occur (be spontaneous)? How do you know? NH3(g) + HCl(g) → NH4Cl(s) ΔH = -176.0 kJ ΔS = -284.8 J•K-1

Solved • Apr 2, 2020

Gibbs Free Energy

Q. ing the given data, determine Δ r S°, Δ r H° and finally Δ r G at 271K for the reaction below. Zn(s) + H2O(g) →ZnO(s) + H2(g) Substance. Δ fH°(kJ/mol-rxn) at 298 K. S° (J/K·mol-rxn) at 298 K. Zn(s) 0 41.6 H2O(g) –241.8 188.7 ZnO(s) –350.5 43.7 H2(g) 0 130.6

Solved • Apr 1, 2020

Gibbs Free Energy

Q. For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data (Due to variations in thermodynamic values for different sources, be sure to use the given values in calculating your answer. ΔH°rxn 180kJ/mol ΔS°rxn 24.08/(mol.K) Calculate the temperature in kelvins above which this reaction is spontaneous. Express your answer to four significant figures and include the appropriate units. The thermodynamic values from part A will be useful as you work through part B: ΔH°rxn 180kJ/mol ΔS°rxn 24.08/(mol.K) Calculate the equilibrium constant for the following reaction at room temperature, 25 °C: N2(g) + O2(g) → 2 NO(g) Express your answer numerically to three significant figures.

Solved • Mar 31, 2020

Gibbs Free Energy

Q. Firefly luciferase is the enzyme that allows fireflies to illuminate their abdomens. Because this light generation is an ATP-requiring reaction, firefly luciferase can be used to test for the presence of ATP. In this way, luciferase can test for the presence of life. The coupled reactions are 1. luciferin + O2 ⇌ oxyluciferin + light 2. ATP ⇌ AMP + PPi ΔG°= -31.6 kJ/mol If the overall ΔG° of the coupled reaction is -5.40 kJ/mol, what is the equilibrium constant, K, of the first reaction at 26 °C? Express your answer numerically.

Solved • Mar 31, 2020

Gibbs Free Energy

Q. Consider these hypothetical chemical reactions: 1. A ⇌ B, ΔG = 14.6 kJ/mol 2. B ⇌ C, ΔG = -26.1 kJ/mol 3. C ⇌ D, ΔG = 5.80 kJ/mol What is the energy, ΔG, for the overall reaction, A ⇌ D? Express your answer with the appropriate units.

Solved • Mar 31, 2020

Gibbs Free Energy

Q. The chemical reaction that causes chromium to corrode in air is given by: 4Cr + 3O2 → 2Cr2O3 In which 298 K ΔH°rxn = -2256 kJ ΔS°rxn = -549.1 J/K At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium? Express your answer as an integer and include the appropriate units.

Solved • Mar 31, 2020