Enter your answer in the provided box. Water gas, a mixture of H2 and CO2, is a fuel made by reacting steam with red-hot coke (a by product of coal distillation): H20(g) +C(s) S CO(g) +H2(g) Using a table of thermodynamic data, estimate the temperature at which the reaction begins to favor the formation of products. °C

Consider the decomposition of methanol, as follows. 2 CH3OH(l) → 2 CH4(g) + O2(g) Suppose 200.0 mL of liquid methanol decomposes at 298 K.  The density of methanol is 0.792 g/mL. What is ξ and ΔH if Δr​H = 327.7kj/mol? Hint: ΔH=ξ×Δr​H

What is the temperature range in which the following reaction is spontaneous? N₂+ 3H2 → 2NH3 S N2(g) 191.5 J/mol K S H2(g) 130.6 J/mol K S NH3(g) 192.5 J/mol K AH, N2(g) 0 kJ/mol AH, H2(g) 0 kJ/mol AH, NH3(g) -46.19 kJ/mol

Consider the reaction given below. H2(g) + F2(g)  2 HF(g) (a) Using thermodynamic data from the course website, calculate G° at 298 K. kJ(b) Calculate G at 298 K if the reaction mixture consists of 5.3 atm of H2, 3.7 atm of F2, and 0.41 atm of HF. kJ

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. MgCl₂ (s) + H₂O(1) AH;xn= V → B MgO(s) + 2 HCl(g) MacBook Air H N M 1 9 DD $10 P m kJ

Calculate AS°rxn for the following reaction. The S° for each species is shown below the reaction. N2H4(l) + H2(g) → 2 NH3(g) ings S°(J/(mol·K)) 121.2 130.7 192.8 O -59.1 J/K es O 311.0 J/K O 133.7 J/K O -133.7 J/K O 637.5 J/K

∆Gº for the reaction, H2(g)+Br2(g)⇄2HBr(g), is -33.3 kJ. Which statement below is true?   To make this reaction go forward, 33.3 kJ must be added.   This reaction is non-spontaneous.   This reaction is spontaneous.   This reaction cannot be at equilibrium.

A mixture of CO(g) and H2(g) is produced by passing steam over hot charcoal: H2O(g)+ C(s)->H2(g)+CO(g) Using the appropriate thermodynamic values in the table below, calculate the lowest temperature at which the reaction is spontaneous under standard conditions. Compound ΔGf (kJ/mol) ΔHf (kJ/mol) ΔHf (kJ/mol) H2O(g) –228.6 –241.8 188.8 H2O(ℓ) –237.2 –285.8 69.9 C(s) 0.0 0.0 5.7 H2(g) 0.0 0.0 130.6 CO(g) –137.2 –110.5 197.7 O2(g) 0.0 0.0 205.0 _____K

Consider the reaction below for the decomposition of carbon tetrachloride gas:  CCl4(g)    ------>     C(s)     +        2Cl2 (g)    ΔH = + 95.7 kJ;  ΔS = + 142.2 J/K  If the reaction above is not spontaneous at 25 oC, determine at what temperature (if any) the reaction becomes spontaneous.

For a particular reaction, Δ?=−14.20 kJ and Δ?=−198.5 J/K. Calculate Δ? for this reaction at 298 K