Consider the reaction P4010(s) + 6H₂O(1) 4H3PO4(aq) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.59 moles of P4010(s) react at standard conditions. AS surroundings J/K
Q: A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a…
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Q: CaO(s) + 2HCI(g) → CaCl₂(s) + H₂O(l) AS⁰ = C₂H4(g) + H₂(g) →C₂H6(g) AS⁰ = J/K J/K
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Q: Consider the reaction Fe(s) + 2HCl(aq) → FeCl2 (s) + H₂(g) for which AH° = -7.400 kJ and AS° = 107.9…
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Q: Which of the following would be expected to have the greatest standard molar entropy at 298K? Ca (s)…
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Q: A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a…
A: If for a reaction ∆G= -ve => forward rxn is spontaneous ∆G= +ve => reverse rxn is spontaneous…
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Q: 2NH₂(g) → N₂(g) + 3H₂(g) ΔΗ = 92. kJ AS = J K AG 25. kJ Which is spontaneous? this reaction the…
A: Given : For first reaction : ∆H = 92. kJ ∆G = 25. kJ Temperature = 70 °C = 343 K For second…
Q: A chemical engineer is studying the two reactions shown in the table below. In each case, she fills…
A: Given that Temperature = T = 150.0 °C = 150.0 + 273.15 = 423.15 K We know that ΔG = ΔH – TΔS…
Q: The
A: We will calculate ∆S
Q: CO₂(g) + 2H₂O(g) → CH₂(g) +20₂ (g) C6H₁₂O6 (s)→ 6C(s) + 6H₂(g) + 30₂ (g) An AS = 2766. AG = KJ Which…
A: Given that: Temperature = 28.0oC For the first reaction ; ∆H = 803 kJ ∆S = 2766 J/K For the second…
Q: ΔΗ 1353. kJ J AS = K 2co,() + 4H,0 (g) → 2CH,OH (g) + 30,(g) AG = 10. kJ Which is spontaneous? this…
A: Given , temperature, T =123°C = (123 +273 )K=396 K Pressure = constant
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Q: Consider the reaction: 2Na(s) + 2H₂O(1) → 2NaOH(aq) + H₂(g) Using standard thermodynamic data at 298…
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Q: A chemical engineer is studying the two reactions shown in the table below. In each case, she fills…
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Q: A chemical engineer is studying the t wo reactions shown in the table below. In each case, she fills…
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Q: A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a…
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Q: Use standard molar entropies to calculate the entropy change (in J/K.mol) for the reaction…
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Q: Using the standard molar entropies, calculate the standard entropy change, AS', for the following…
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Q: A chemical engineer is studying the two reactions shown in the table below. In each case, she fills…
A: ∆G and ∆S can be calculated using formula : ∆G = ∆H - T∆S To check the spontaneity , we use the…
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A: Recall the given reactions, 3 CO2 g + 4 H2O l → C3H8 g + 5 O2 g…
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Q: A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a…
A: The formula used here is, ∆G = ∆H - T∆S ∆G = Gibbs free energy of a reaction ∆H = reaction enthalpy…
Q: A chemical engineer is studying the two reactions shown in the table below. In each case, she fills…
A: Answer: In this question on the basis of value of ∆G we have to decide which reaction is spontaneous…
Q: Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your…
A: The relationship between ∆G, ∆H and ∆S is as follows: ∆G=∆H - T∆S ∆H is change in enthalpy of…
Q: A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a…
A: A reaction in which the change in Gibbs free energy is negative or less than zero is a spontaneous…
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Q: Using the standard molar entropies, calculate the standard entropy change, AS°, for the following…
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A: Given, (a). P4 (g) + 6Cl2 (g) --------> 4PCl3 (g) Change in enthalpy of the reaction = ΔH =…
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A: As we know, ∆G = ∆H - T∆S A reaction is Spontaneous if ∆G is negative. While reverse reaction is…
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Q: Consider the reaction: 2Na(s) + 2H₂O(1)→ 2NaOH(aq) + H₂(g) Using standard thermodynamic data at 298…
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Q: A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a…
A: Temperature , T = 72.0 °C=(72+273)K=345 K
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Q: Which is spontaneous? this reaction
A: Given temperature = 144.0°C Given two reaction C3H8g + 5O2g ---> 3CO2g+ 4H2O ΔH= −2220.kJ ΔS =…
Q: A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a…
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- Using the provided data, determine the temperatures at which the following hypothetical reaction will be spontaneous under standard conditionsA + B → 2C + D△S°rxn = 249.1 J/K△H°rxn = 104.6 kJ * at no temperatures * at all temperatures below 146.9 °C * at all temperatures above 146.9 °C * at all temperatures above 238.1 °C * at all temperatures below 238.1 °C * at all temperaturesA chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 61.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy as of the first reaction, and the reaction enthalpy H and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and As for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 4H₂O₂(1) + PbS (s) PbSO₂ (s) + 4H₂0 (1) Sn (s) + 2CO₂ (g) SnO₂ (s) + 2CO (g) ΔΗ = - 1212. kJ AS = -3559. AG = KJ Which is spontaneous? Othis reaction O the reverse reaction O neither…A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 26.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. N₂(g) + 3H₂(g) → 2NH₂(g) P₁(s) + 20HF (g) 4PF, (g) + 10H₂(g) ΔΗ = -92. kJ AS = AG = | KJ -294. ΔΗ Which is spontaneous? this reaction the reverse reaction neither AS = = - 1005. kJ…
- A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 69.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. HCH, CO₂(1)→ CH₂OH(g) + CO(g) Al₂O₂ (s) + 2Fe(s) -> 2A1(s) + Fe₂O₂ (s) AH = 172. kJ AS = 543. AG = Which is spontaneous? O this reaction O the reverse reaction Oneither ΔΗ = 852. kJ…A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 114.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. ol. Ar AH = 852. kJ J AS = 2176. Al, 0, (s) + 2Fe(s) → 2 A1(s) + Fe,0, (s) AG = | kJ Which is spontaneous? this reaction the reverse reaction neitherA chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 100.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2Al(s) + 3H₂O(g) → Al₂O₂ (s) + 3H₂(g) 2CO₂(g) + 4H₂O(g) → 2CH₂OH(g) + 30₂ (g) ΔΗ = -951. kJ AS = -2549. AG = | KJ -0-/21 K Which is spontaneous? this reaction the reverse reaction…
- Consider the reaction Fe(s) + 2HCl(aq) → FeCl₂ (s) + H₂(g) for which AH = -7.400 kJ and AS = 107.9 J/K at 298.15 K. 1. Calculate the entropy change of the UNIVERSE when 2.385 moles of Fe(s) react under standard conditions at 298.15 K. ASuniverse J/K 2. Is this reaction reactant or product favored under standard conditions? 3. If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'. Submit Answer Retry Entire Group 5 more group attempts remainingConsider the reaction: 6CO2(g) + 6H₂O(l) → C6H12O6 + 602 (9) Using standard thermodynamic data at 298 K, calculate the entropy change for the surroundings when 1.87 moles of CO₂ (g) react at standard conditions. AS⁰ Substance AH (kJ/mol) CO₂ (g) -393.5 H₂O(1) -285.8 C6H12O6 -1275.0 O₂(g) 0.0 surroundings J/KWhat would the entropy be for a system with 6.05E+1 microstates, in J/mol-K?
- A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 133.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2CH₂OH(g) + 30₂(g) → 2CO₂(g) + 4H₂O(g) 4H₂PO4(s) P4O10 (s) + 6H₂0 (1) AH-1353. kJ AS = -3331. AG = Which is spontaneous? Othis reaction O the reverse reaction Oneither ΔΗ = 439. kJ -…Consider the reaction: NH4Cl(aq) →→→→NH3(g) + HCl(aq) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.90 moles of NH4Cl(aq) react at standard conditions. AS° surroundings = J/KA chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 146.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.