Predict whether the entropy change will be positive or negative for the following reaction.  Justify your answer.   H2C=CH2  +  2 O3    =    6 CH2O

Given the informationR + X → Q + Z ΔH= 165 kJQ + Z → T ΔH= 165 kJ calculate ΔH for each of the following reactions. R+X→T Q+Z→R+X 2Q+2Z→2R+2X

Consider the following reactions. NiSO3(s) →NiO (s) + SO2 (g)        ∆H= 162.0 kJ   SO2 (g) →   1/8 S8(s) + O2 (g)      ∆H= 290.0 kJ     2Ni (s) + O2 (g) → 2NiO (s)          ∆H= -478.0 kJ   A) Calculate ∆H (in kJ) for the reaction. 8Ni (s) + S8(s) + 12O2 (g) →8NiSO3 (s) B) Calculate ∆H (in kJ) for the decomposition reaction of 2.00 g of NiSO3(s) according to the reaction.            8NiSO3 (s)→ 8Ni (s) + S8(s) + 12O2 (g)   C) Carbon tetrachloride (CCl4) was at one time used as a fire-extinguishing agent. The molar heat capacity is 131.3 J/(mol°C). Calculate the amount of energy in kJ required to raise the temperature of 22.0 g of CCl4 from 22.0 °C to 66.0 °C.

Octane 1C8H182 is a liquid hydrocarbon at room temperature that is a constituent of gasoline. Without using thermochemical data, predict whether ∆G° for this reaction is more negative or less negative than ∆H°

Using appropriate experimental data, a researcher calculates their enthalpy and entropy for a reaction as listed below. Calculate the standard Gibbs Free Energy, Δ G ∘, for this reaction in units of kJ mol. Report your final answer to one place after the decimal. Enthalpy = 30.37 kJ/mol Entropy = -3.59 J/mol

Indicate which of the four cases below applies to the following four reactions (a through d) by writing 1, 2, 3, or 4 after each letter Spontaneous at all temperatures. Spontaneous above a certain temperature. Spontaneous below a certain temperature. Non-spontaneous at all temperatures. a)     PCl3(g) +   Cl2(g)   ↔   PCl2(g)                                    ΔH° = -87 KJ        b)     CH4(g) +   2 O2(g)   ↔   CO2(g)   +   2 H2O(g)         ΔH° = +41 KJ      c)     2 NH3(g) →   N2(g)   +   3 H2(g)                                 ΔH° = +160 KJ      d)      Mg(s) +   2 HCl(aq)   →   MgCl2(aq)   +   H2(g)          ΔH° = -462 KJ    please write which number they classify as

Quick overview of our lesson: Our topic is all about Second Law of Thermodynamics. Gibbs’ free energy, G is defined by G = H – TSwhere H is the enthalpy, T is the temperature (in Kelvins), and S is the entropy. In a chemical reaction,R ↔P (R are reactants and P are products) at aconstant temperature we have ∆G = ∆H – T∆S.If ∆G < 0 the reaction may proceed spontaneously tothe right.If ∆G = 0 the reaction is in equilibrium.If ∆G > 0 the reaction may proceed spontaneously to the left. please do help me with the questions on the picture

5. What can be interpreted if only given the following? C6H12O6(s) ----> C6H12O6(aq) The enthalpy of the reaction is negative. The enthalpy of the reaction is positive. The entropy of the reaction is negative. The entropy of the reaction is positive. Not enough information is provided to make any predictions.

Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change A solid absorbs heat and turns to a gas. During an exothermic chemical reaction, a solid is consumed and a gas produced. Is this change spontaneous? Yes. No. Can't decide with information given. ○ Yes. ○ No. Can't decide with information given. An endothermic chemical reaction between two liquids results in gaseous products. Yes. No. ○ Can't decide with information given.

Be sure to answer all parts. Predict whether the entropy change is positive or negative for each of the following reactions. 2 KCIO,(s) →2 KCIO3(s) + O2(g) positive negative H20(g) → H20() positive negative