Question

In: Chemistry

2CH4(g)→C2H6(g)+H2(g) Calculate ΔG∘rxn at 25 ∘C. 2NH3(g)→N2H4(g)+H2(g) Calculate ΔS∘rxn at 25 ∘C. N2(g)+O2(g)→2NO(g) calculate ΔH∘rxn and...

2CH4(g)→C2H6(g)+H2(g) Calculate ΔG∘rxn at 25 ∘C.

2NH3(g)→N2H4(g)+H2(g) Calculate ΔS∘rxn at 25 ∘C.

N2(g)+O2(g)→2NO(g) calculate ΔH∘rxn and Calculate ΔG∘rxn at 25 ∘C.

2KClO3(s)→2KCl(s)+3O2(g) calculate ΔH∘rxn .and Calculate ΔG∘rxn at 25 ∘C.

Expert Solution

2CH4(g)→C2H6(g)+H2(g) Calculate ΔG∘rxn at 25 ∘C.

dG = Gproducts - Greactants

dG = (C2H6 + H2) - (2CH4)

dG = -32.0 + 0 - 2(-50.5) kJ/mol

dG = 69 kJ/mol

2NH3(g)→N2H4(g)+H2(g) Calculate ΔS∘rxn at 25 ∘C.

dS = Sprod - Sreact

dS = N2H4 + H2 - (2NH3)

dS = (121.2 + 130.7) - (2*(192.8))

dS = -133.7 J/molK

N2(g)+O2(g)→2NO(g) calculate ΔH∘rxn and Calculate ΔG∘rxn at 25 ∘C.

dH = Hprod - Hreact

dH = 2*NO - (N2 + O2)

dH = 2*91.3 - (0 + 0)

dH = 182.6 kJ/mol

fo dG

dG = Gprducts - Greactands

dG = 2*NO - (N2 + O2)

dG = 2*87.6 - (0 +0)

dG = 175.2 kJ/mol

2KClO3(s)→2KCl(s)+3O2(g) calculate ΔH∘rxn .and Calculate ΔG∘rxn at 25 ∘C.

dH= Hprod - Hreact

dH = (2KCl + 3O2) - (2KClO3)

dH = (2*-436.5+3*0 -(2*-397.7)

dH = -77.6 kJ/mol

dG= Gprod - Greact

dG = (2KCl + 3O2) - (2KClO3)

dG = 2*-408.5 + 3*0 - (2*-296.3)

dG = -224.4 kJ/mol

queen_honey_blossom answered 2 years ago

1)For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. 3H2(g)+Fe2O3(s)→2Fe(s)+3H2O(g) N2(g)+3H2(g)→2NH3(g)...

1)For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. 3H2(g)+Fe2O3(s)→2Fe(s)+3H2O(g) N2(g)+3H2(g)→2NH3(g) 2)Before investigating the scene, the technician must dilute the luminol solution to a concentration of 6.00×10−2M . The diluted solution is then placed in a spray bottle for application on the desired surfaces. How many moles of luminol are present in 2.00 L of the diluted spray? 3)A student placed 11.0 g of glucose (C6H12O6) in a volumetric flask, added enough water to dissolve...

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether...

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C?2CH4(g)→C2H6(g)+H2(g), Calculate ΔS∘rxn at 25 ∘C. 2NH3(g)→N2H4(g)+H2(g) Calculate ΔS∘rxn at 25 ∘C. N2(g)+O2(g)→2NO(g) Calculate ΔS∘rxn at 25 ∘C. 2KClO3(s)→2KCl(s)+3O2(g) Calculate ΔS∘rxn at 25 ∘C.

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, ΔG∘rxn at 25 ∘C. State whether or...

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C? a) 2CH4(g)→C2H6(g)+H2(g) b) 2NH3(g)→N2H4(g)+H2(g) c) N2(g)+O2(g)→2NO(g) d) 2KClO3(s)→2KCl(s)+3O2(g) Can you please show equations. I am having so much trouble with these.

Calculate ΔG∘rxn for the following reaction: 4CO(g)+2NO2(g)→4CO2(g)+N2(g). Use the following reactions and given ΔG∘rxn values: 2NO(g)+O2(g)→2NO2(g),...

Calculate ΔG∘rxn for the following reaction: 4CO(g)+2NO2(g)→4CO2(g)+N2(g). Use the following reactions and given ΔG∘rxn values: 2NO(g)+O2(g)→2NO2(g), ΔG∘rxn= - 72.6 kJ 2CO(g)+O2(g)→2CO2(g), ΔG∘rxn= - 514.4 kJ 12O2(g)+12N2(g)→NO(g), ΔG∘rxn= 87.6 kJ

Calculate the ΔG°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) → 7 N2(g) +...

Calculate the ΔG°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) → 7 N2(g) + 12 H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -133.9 50.6 -285.8 S°(J/mol • K) 266.9 121.2 191.6 70.0

1. Calculate delta S at 27*c: 2CH4 (g) --> C2H6 (g)+ H2 (g) 2. Calculate delta...

1. Calculate delta S at 27*c: 2CH4 (g) --> C2H6 (g)+ H2 (g) 2. Calculate delta S at 27*c: 2NH3 (g) --> N2H4 (g) + H2 (g) 3. If delta H (+) and delta S (-) is it spontaneous?

Determine ΔH°rxn at 25 °C for the reaction 2 HCN(g) → 2 C(graphite) + H2(g) +...

Determine ΔH°rxn at 25 °C for the reaction 2 HCN(g) → 2 C(graphite) + H2(g) + N2(g) given that the standard heat of formation (ΔH°f) of HCN(g) is 135.1 kJ/mol

For each of the following reactions, calculate ΔH∘rxnΔHrxn∘, ΔS∘rxnΔSrxn∘, and ΔG∘rxnΔGrxn∘ at 25 ∘C∘C. State whether...

For each of the following reactions, calculate ΔH∘rxnΔHrxn∘, ΔS∘rxnΔSrxn∘, and ΔG∘rxnΔGrxn∘ at 25 ∘C∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C∘C? Part A 2CH4(g)→C2H6(g)+H2(g)2CH4(g)→C2H6(g)+H2(g) Express your answer to one decimal place. Part B Calculate ΔS∘rxnΔSrxn∘ at 25 ∘C∘C. Express your answer to one decimal place. Part D 2NH3(g)→N2H4(g)+H2(g)2NH3(g)→N2H4(g)+H2(g) Express your answer to one...

Estimate ΔG°rxn for the following reaction at 407 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH°=...

Estimate ΔG°rxn for the following reaction at 407 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH°= -158.0 kJ; ΔS°= -219.9 J/K answer choices -68.5 kJ +247 kJ -247 kJ +68.5 kJ +61.9 kJ

Consider the reaction N2(g) + 3H2(g) → 2NH3(g)ΔH o rxn = −92.6 kJ/mol If 2.0 moles...

Consider the reaction N2(g) + 3H2(g) → 2NH3(g)ΔH o rxn = −92.6 kJ/mol If 2.0 moles of N2 react with 6.0 moles of H2 to form NH3, calculate the work done (in joules) against a pressure of 1.0 atm at 25 degrees celsius. What is ΔU for this reaction? Assume the reaction goes to completion.