2. Observe the Figure 2.0, in which there are 4 types of reactions. Using the definition of Gibbs' free energy. Identify which is a spontaneous reaction and explain why on the space provided. REACTION TYPE ONE AH TAS TAS AG REACTION TYPE TWo AH TAS -TAS AG REACTION TYPE THREE AH TAS -TAS AG REACTION TYPE FOUR AH TAS -TAS AG Figure 2.0. Four types of Reaction described according to thermodynamic properties.

Q: Calculate ΔrH° for the combustion of methane gas, CH4 : CH4(g)  +   2 O2(g)  →   CO2(g)  +  2…

A: Given  CH4(g)  +   2 O2(g)  →   CO2(g)  +  2 H2O(g) molecule                                  ΔfH°…

Q: Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation…

A:

Q: Determine ΔrH° in kJ/mol for the reaction,  4 NO(g) + 6 H2O(g) →4 NH3(g) + 5 O2(g) using the…

A:

Q: Quick overview of our lesson: Our topic is all about Second Law of Thermodynamics. Gibbs’ free…

A: Gibb's free energy of the reaction is an important parameter in deciding the spontaneity of the…

Q: ( in kilojoules) for the industrial synthesis of chloroform (CHCl3) in a reaction of methane ( CH4)…

A:

Q: Write the CAPITAL Letter of the correct answer. A if both statements are true  B if the 1st…

A: Given that, two statements are If the change in free energy, ΔG is negative, the reaction is…

Q: Oxyacetylene torches produce such high temperature that they are often used to weld and cut metal.…

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Q: Calculate the ∆H°rxn for the reaction C(graphite) + 2H2(g) → CH4(g) from the following enthalpy…

A: ∆H°rxn can be calculated from the enthapy change of the given reactions. If the reaction is…

Q: The balanced chemical equation for the combustion of propane gas is: C3H8 (g) + 5 O2 (g) --> 3 CO2…

A:

Q: Consider the following reaction at 298 K: 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) Suppose 150 g of iron…

A: The balanced equation is: 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) ; ∆Ho = ??  First, we have to find the…

Q: Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is…

A: Heat given Q = 25.0 kJ  Initial volume Vi = 12.00 L  Final volume Vf = 6.00 L Constant pressure P =…

Q: 2. The muscles in our bodies work similar to that of a fuel cell, by metabolizing sugar (glucose) to…

A: Given: standard enthalpy of formation of glucose (s) = -1273.3kJ/mol standard enthalpy of formation…

Q: Sulfur dioxide reacts with oxygen to produce sulfur trioxide. Thermodynamic Data Substance ΔfH∘…

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Q: For a particular reaction at 148.1 °C, Δ?=−1428.51 kJ, and         Δ?=393.69 J/K  .  Calculate Δ?…

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Q: 4. Find the standard molar enthalpy for the reaction Cos+ ½ Oxg}→ COe Co+ Oz→ C0xg AH = -394 kJ CO2…

A: Given: (i) C(s) + ½ O2(g) → CO(g)                          ;  ΔH°(i) (ii) C(s) + O2(g) → CO2(g)…

Q: Determine ΔrH° in kJ/mol for the reaction,  4 NO(g) + 6 H2O(g) →4 NH3(g) + 5 O2(g) using the…

A:

Q: Given the following: P,(s) + 50,(g) → P,0,(s) A G° = – 2697.0 kJ/mol2H, (g) +0,(g) → 2H,0(g) A G° =…

A:

Q: Using the following reactions: NO (g) + 0.5 O 2 (g) --> NO 2 (g)             ∆H = 50 kJ x    N 2O 4…

A: Determine  the enthalpy change of the given reaction.

Q: Observe the Figure 1.0 in which the influence of temperature to change in enthalpy, ∆H and entropy,…

A: Each chemical reaction is associated with a certain amount of energy. This energy can be liberated…

Q: Consider a 1.2 mol block of iron with a specific heat capacity of 0.44 J/g°C. The atomic mass of Fe…

A: The amount of heat required to raise the temperature of the sample is given by: q =m c∆Tq is the…

Q: Use the Standard Thermodynamic Properties table to calculate ΔHo for the following reaction:…

A: Thermodynamic is the branch of chemistry that mainly deals with the heat transfer between system and…

Q: which reaction of carbon monoxide w metal oxide would produce pure metal and carbon dioxide…

A: The reactions given are, 1) Fe2O3(s)  →  2 Fe(s)  +  3/2 O2(g)          ΔrGº = +742.2 KJ/mol  2)…

Q: 6) Consider H;0 going from the gas phase to liquid phase to solid phase. Describe the changes in…

A: In the vapor state, the gas phase of water, water molecules have the highest kinetic energy and this…

Q: Observe the Figure 1.0 in which the influence of temperature to change in enthalpy, ∆H and entropy,…

A: The change in heat content associated with a chemical reaction is denoted by the term enthalpy…

Q: The balanced chemical equation for the combustion of propane gas is: C3H8 (g) + 5 O2 (g) --> 3 CO2…

A: Given reaction: C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g) ∆G°RXN = -2385 kJ Temperature = 17.0 °C…

Q: Calculate ΔHrxn for the reaction using the following data. Target Reaction:    WO3 (s) + 3H2 (g) →…

A: The reactions given are 1) W (s) + 3/2 O2 (g) → WO3 (s)                ΔH = ‒842.7 kJ 2) H2 (g) +…

Q: ce AH°rxn for ΔΗ

A:

Q: ∆H rxn

A:

Q: The value of ΔE in kJ, for a system that does 213 kJ of work on its surroundings and loses 79 kJ of…

A:

Q: Calculate the standard enthalpy change for the following reaction at 25 °C. MgCl, (s) + H,O(1)…

A:

Q: ENTROPY (ΔS) can be thought of as molecular disorder, randomness, or freedom. Which of the two…

A: Entropy measures the disorder or randomness in the system. Ice has more ordered structure than…

Q: he balanced chemical equation for the combustion of propane gas is: C3H8 (g) + 5 O2 (g) --> 3 CO2…

A: The standard free energy (G) and the Gibbs free energy change (∆G°) can be related by the equation…

Q: Consider the vaporization of 1 mol of a liquid,  A(l) ⟶⟶A(g)  at 298 K and 1.00 atm.  If 39.5 KJ…

A:

Q: Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation…

A: The standard conditions are:  Product ∆Hf KJ/mol Mg(OH)2 s   -924.7 HCl(g) -92.5 Mg(Cl)2 s…

Q: true? Select one: Exothermic processes decrease the entropy of the surroundings. The standard molar…

A: We will pick Correct statement

Q: Calculate the standard free energy change for the combustion of 1 mole methane using standard free…

A: Given that :

Q: What is the significance of the change in Gibbs free energy (∆G)for a reaction?

A: The significance of the change in Gibbs free energy (∆G)for a reaction: (i) If ∆G for a reaction…