Using enthalpies of formation, calculate deltaH for the following reaction at 25°C. Also calculate deltaS for this reaction from standard entropies at 25°C. Use these values to calculate deltaG for the reaction at this temperature. Species  deltaHf(kJ/mol)  S(J/mol⋅K) CH3OH(l) –238.7 126.8 O2(g) 0 205.0 CO2(g) –393.5 213.7 H2O(l) –285.8 69.95 2CH3OH(l) +3O2(g) --- 2CO2(g) + 4H2O(l) deltaH =  kJ deltaS =  J/K deltaG =  kJ

Use the References to access important values if needed for this question. -87.9 kJ, and Kc Consider the following system at equilibrium where AH 500 K: = The value of Qc Ois greater than K O is equal to Ke O is less than Ke = PC13 (g) + Cl₂ (g) ⇒ PC15 (9) When 0.36 moles of PC15 (9) are added to the equilibrium system at constant temperature: The value of Kc Oincreases decreases O remains the same The reaction must Orun in the forward direction to reestablish equilibrium run in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of PC13 will O increase decrease O remain the same 83.3, at Previou

For the reaction A (g) → 2B (g), K = 14.7 at 298 K. What is the value of Q for this reaction at 298 K when AG = -20.4 kJ/mol?

Consider the following equilibrium: +N2g3H2g    2NH3g =       ΔG0−34.kJ Now suppose a reaction vessel is filled with  2.58atm  of nitrogen  N2  and  3.27atm  of ammonia  NH3  at  647.°C . Answer the following questions about this system: Under these conditions, will the pressure of  NH3  tend to rise or fall?   rise     fall   Is it possible to reverse this tendency by adding  H2 ?In other words, if you said the pressure of  NH3  will tend to rise, can that be changed to a tendency to fall by adding  H2 ? Similarly, if you said the pressure of  NH3  will tend to fall, can that be changed to a tendency to rise by adding  H2 ?   yes     no   If you said the tendency can be reversed in the second question, calculate the minimum pressure of  H2  needed to reverse it.Round your answer to  2  significant digits. atm

Consider the following reaction:Cu2S (s) + O2 (g) ⇌ 2Cu (s) + SO2 (g) 1.1 Determine the estimated value of the equilibrium constant for this reaction at 200 `C by making use of the following data: Is the reaction reactant- or product favoured atthis temperature? Use a short sentence to explain your answer. 1.3 Calculate the value of ΔrG for this reaction at this temperature, if O2 and SO2 are present at 0.900 atm and 0.800 atm, respectively. Substance  S° (Jmol. K) at 25 'C ∆fH° (kj mol) at 25 'C Cu2S(?) 120.9  -79.5 O2(?) 205.0  0 Cu(s) 33.1  0  SO2(g) 248.1 -296.8 Please answer Question 1.1

At a certain temperature, 523 K, Kp for the reaction,N2O4(g) <=> 2 NO2(g), is 4.15 x 10-50.Calculate the value of ΔGo in kJ for the reaction at 523 K.

Use the table of thermodynamic values to calculate the value of ΔG°rxn at 25.0 °C for the reaction      2 HCl (g)  +  F2 (g)    ⇌    2 HF (g)  +  Cl2 (g) Then, use your calculated value of ΔG°rxn to find the equilibrium constant at 25.0 °C for this reaction.

A 80.0 mL sample of 0.300 M aqueous hydrochloric acid is added to 80.0 mL of 0.300 M aqueous ammonia in a coffee cup calorimeter. The following reaction occurs when the two solutions are mixed: HCl(aq) + NH3(aq) → NH4Cl(aq) The temperature of the solution increases by 4.30°C. Calculate ΔrH per mole of HCl and NH3 reacted. Assume no heat is lost to the calorimeter, and the density and specific heat capacity of the solution is that of pure water (d=1 g/mL, Cs = 4.18 J/gK). Express your answer in kJ mol-1 to 3 significant figures.

Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH,(g) → 3 Ni(s) + N,(g) + 3 H,O(g) K If AH° = 85.7 kJ/mol and AS° = 348.3 J/mol•K, estimate the temperature at which this reaction would be at equilibrium assuming that enthalpy and entropy are independent of temperature. %3D 1 6. C 7 8 9. +/- x 100 3. 2. 4.

Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. Mg(OH), (s) + 2 HCI(g) MgCl, (s) + 2 H,O(g) AHn = kJ