Carbonyl fluoride, COF2, is a chemical reagent useful in the synthesis of fluorinated organic compounds. The decomposition of COF2 occurs at high temperature and with a catalyst according to the following reaction: Part A 2 COF2(g) = CO2(g) + CF4(g) Determine the equilibrium constant at 675 K. Given that A,H = -47.5 kJ mol-1 and the equilibrium constant at 852 K is K = 7.14: O 7.13 O 7.16 O 1.23 34.6 O 41.5

Please show the complete solution.

If 50.0 g of H₂ and 125.5 g of O₂ react, how many moles of H₂O can be produced in the reaction below? 2 H₂(g) + O₂(g) → 2 H₂O(g)

Write a balanced standard formation reaction and a balanced standard combustion reaction for each of the following compounds, and For each of the compounds in Q-9, calculate the standard enthalpy of combustion using enthalpies of formation from the table of thermodynamic properties  a) CH4 (methane)  b)  C6H12O6 (s) [ glucose ]

A chemical engineer is studying the following reaction: BF3(aq)+NH3(aq) → BF3NH3(aq) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 1.1. The engineer charges ("fills") three reaction vessels with boron trifluoride and ammonia, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound concentration expected change in concentration BF 3 0.64 M O f increase OI decrease O (no change) A NH, 0.90 M O f increase OI decrease O (no change) BF;NH; 0.63 M O f increase O! decrease (no change) BF3 0.84 M O f increase O! decrease O (no change) В NH, 1.19 M O f increase OI decrease O (no change) BF;NH, 1.09 M O 1 increase OI decrease (no change) BF3 0.38 M O t increase OI decrease O (no change) NH, 0.64 M O t…

Consider the following dissolution of lead(II) fluoride (PbF>(s): O 5.9 kJ molr1 PbF>(s) - Pb2*(ag) + 2 F(ag) O 5.9 kJ mol1 Below is a table of thermodynamic quantities pertaining to this reaction: Submit Request Answer Substance AHP (kJ mol1) S° (J K-1 mol1) Part B PBF2(s) -664.0 110.5 Determine the standard entropy of reaction (A,S°) for the dissolution of lead(II) fluoride. Pb2*(aq) 0.9 18.5 O 119.6 J K1 mol1 F(ag) -335.4 -13.8 O -105.8 J K1 mor1 O 119.6 J K1 mor1 O 105.8 J K-1 mol1

A solid mixture containing MgSO4 is dissolved in water and treated with an excess of Ba(NO3)2, resulting in the precipitation of 0.6 g of BaSO4.The molecular weight of BaSO4 is 233 g/mol. Number of moles of MgSO4 in the mixture is? O 0.00257mol O 0.52700 mol O 0.05720 mol O 0.25700 mol O 0.02570 mol

For the following reaction at equilibrium in a reaction vessel, which one of the changes below would cause the Br2 concentration to decrease?   2NOBr(g)   ↔   2NO(g) + Br2(g)         ΔH= 30 kJ/mol     Increase the temperature     Remove some NO     Add more NOBr     Compress the gas mixture into a smaller volume

Balance the following redox reaction in an acidic solution: UO22+(aq)+Zn(s)->U4+(aq)+Zn2+(aq)

26.20 The data provided in Figure 26.7 are based on the diffusion of O₂ into SiO₂ formed from the oxidation of (100) crystalline silicon at 1000°C. Estimate the diffusion coefficient of O₂ in SiO₂ formed from the oxidation of (111) crystalline silicon at 1000 °C, using the data in the table below, provided by Hess (1990).* Time 1.0 2.0 4.0 7.0 16.0 Measured SiO₂ Film Thickness (um) 0.049 0.078 0.124 0.180 0.298 0.070 0.105 0.154 0.212 0.339 The maximum solubility of O₂ in the SiO₂ is 9.6-10-8 mole 0₂/cm³ solid at 1000°C and 1.0 atm O₂ gas partial pressure. *D.W. Hess, Chem. Eng. Education, 24, 34 (1990).