Need the answer to part BHomework Answers
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Need the answer to part B
The decomposition of crystalline N, O N,Og(s) + 2NO2(g) +...
The decomposition of crystalline N2O5 N2O5 (s) —> 2 NO2 (g) + 1/2 O2 (g) is...
The decomposition of crystalline N2O5 N2O5 (s) —> 2 NO2 (g) + 1/2 O2 (g) is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25°C we have the following values for the standard state entrapped and free energy changes of the reaction: ΔH° = +109.6 kJ/mol ΔG° = -30.5 kJ/mol a. Calculate ΔS° at 25°C b. Why is the entropy change so favorable for this reaction? Please answer and explain both questions!
The decomposition of crystalline N2O5 N2O5(s)⟶2NO2(g)+12O(g) is an example of a reaction that is thermodynamically favored...
The decomposition of crystalline N2O5 N2O5(s)⟶2NO2(g)+12O(g) is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25 ∘C we have the following values for the standard state enthalpy and free energy changes of the reaction: ΔH∘=+109.6kJ/mol ΔG∘=−30.5kJ/mol c. What is driving the reaction forwards: enthalpy, entropy or both?
To answer Questions 2.1-2.4, you will need the thermodynamic data below. SPECIES A | B |...
To answer Questions 2.1-2.4, you will need the thermodynamic data below. SPECIES A | B | C | D. | AH1° 0 kJ/mol 0 kJ/mol | +185 kJ/mol -360 kJ/mol | Note that the letters should not be interpreted as elemental symbols (for example, "C" does not stand for "carbon"), but rather treated as variables standing in for species of unknown identity. 2.1. Calculate the enthalpy change for the reaction below. Express your answer in kJ/mol C rounded to the...
B. Calculate the standard entropy change for the reaction 2Na(s)+Cl2(g)?2NaCl(s) using the data from the following t...
B. Calculate the standard entropy change for the reaction
2Na(s)+Cl2(g)?2NaCl(s)
using the data from the following table:
Substance
?H?f (kJ/mol)
?G?f (kJ/mol)
S? [J/(K?mol)]
Na(s)
0.00
0.00
51.30
Cl2(g)
0.00
0.00
223.1
NaCl(s)
-411.0
-384.0
72.10
Express your answer to four significant figures and include the
appropriate units.
Part A Predict the sign of the entropy change, AS°,for each of the reaction displayed. Drag the appropriate items to their respective bins. Ag+(aq) + Cl-(aq) → AgCl(s) | | Ca(OH)2(s) →...
H2 reacts with the halogens (X2) according to the reaction: H2 (9) + X2 (g) =...
H2 reacts with the halogens (X2) according to the reaction: H2 (9) + X2 (g) = 2HX (9) where X2 can be Cl2, Br2 , or 12. Reactant/Product AH; (kJ/mol) AS; (J/mol · K) H2(9) 130.7 223.1 HCl(9) -92.3 186.9 30.9 245.5 HBr(9) -36.3 198.7 12(9) 62.42 260.69 HI(9) 26.5 206.6 Cl2(9) Br2(9) Part L Calculate K, for the reaction between hydrogen and I2. Express your answer using three significant figures. EVO AED Om ? Кр: Submit Request Answer Part...
ormation Reactions Review Constants Part B The standard heat of formation, AH is defined as the...
ormation Reactions Review Constants Part B The standard heat of formation, AH is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have AH O . Heat of formation values can be used to calculate the enthalpy change of any reaction. The combustion of propano, C, Hs. cocurs via the reaction CH, (B) +502 (6)+3CO2 (s) + 4H2O(g) with heat of formation...
< 9 of 13 Review Constants Periodic Table Part A A calorimeter contains 28.0 mL of...
< 9 of 13 Review Constants Periodic Table Part A A calorimeter contains 28.0 mL of water at 11.0 °C. When 250 g of X (a substance with a molar mass of 60.0 g/mol) is added, it dissolves via the reaction X(s) + H2O(1) X(aq) and the temperature of the solution increases to 30.0 °C. Calculate the enthalpy change, AH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that...
To answer Questions 2.1-2.4, you will need the thermodynamic data below. SPECIES A | B | C | D. | AH1° 0 kJ/mol 0 kJ/mol | +185 kJ/mol -360 kJ/mol | Note that the letters should not be interpreted as elemental symbols (for example, "C" does not stand for "carbon"), but rather treated as variables standing in for species of unknown identity. 2.1. Calculate the enthalpy change for the reaction below. Express your answer in kJ/mol C rounded to the...
B. Calculate the standard entropy change for the reaction
2Na(s)+Cl2(g)?2NaCl(s)
using the data from the following table:
Substance
?H?f (kJ/mol)
?G?f (kJ/mol)
S? [J/(K?mol)]
Na(s)
0.00
0.00
51.30
Cl2(g)
0.00
0.00
223.1
NaCl(s)
-411.0
-384.0
72.10
Express your answer to four significant figures and include the
appropriate units.
Part A Predict the sign of the entropy change, AS°,for each of the reaction displayed. Drag the appropriate items to their respective bins. Ag+(aq) + Cl-(aq) → AgCl(s) | | Ca(OH)2(s) →...
H2 reacts with the halogens (X2) according to the reaction: H2 (9) + X2 (g) = 2HX (9) where X2 can be Cl2, Br2 , or 12. Reactant/Product AH; (kJ/mol) AS; (J/mol · K) H2(9) 130.7 223.1 HCl(9) -92.3 186.9 30.9 245.5 HBr(9) -36.3 198.7 12(9) 62.42 260.69 HI(9) 26.5 206.6 Cl2(9) Br2(9) Part L Calculate K, for the reaction between hydrogen and I2. Express your answer using three significant figures. EVO AED Om ? Кр: Submit Request Answer Part...
ormation Reactions Review Constants Part B The standard heat of formation, AH is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have AH O . Heat of formation values can be used to calculate the enthalpy change of any reaction. The combustion of propano, C, Hs. cocurs via the reaction CH, (B) +502 (6)+3CO2 (s) + 4H2O(g) with heat of formation...
< 9 of 13 Review Constants Periodic Table Part A A calorimeter contains 28.0 mL of water at 11.0 °C. When 250 g of X (a substance with a molar mass of 60.0 g/mol) is added, it dissolves via the reaction X(s) + H2O(1) X(aq) and the temperature of the solution increases to 30.0 °C. Calculate the enthalpy change, AH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that...
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