Acetaldehyde is produced from the input components CH4 and CO according to the following CH4(g) +CO(g) ⇒CH₂CHO(g) K673 K = 6.23 CH4 and CO are initially present in the reaction medium in stoichiometric amounts, and for every 1 mole of CO, 4 moles of nitrogen gas are fed to the reactor. Calculate the composition values of the equilibrium mixture based on the reactor reaching equilibrium at 673 K and 100 bar conditions. The gas phase in equilibrium shows ideal solution behavior. gas phase catalytic reaction:

can you help with A and B    My high school teacher said this is a good practice problem

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

Problem 3. One way to produce formaldehyde (HCHO) is via the partial oxidation of methanol (CH3OH). However, when methanol reacts with oxygen, some of the methanol is instead converted to carbon dioxide, and some methanol is converted to formic acid (HCOOH). Note, not more than one of these three products is created in the same reaction, but in every reaction, water is a byproduct. Suppose that 100 kmol/hr methanol and 50 kmol/hr of oxygen are fed to a reactor. Analysis of the reactor effluent reveals 62.5 kmol/ht of methanol, 10 kmol/hr of oxygen, and 57.5 kmol/hr of water exits. (b) Write the three balanced chemical reactions involved in this process. (c) Complete a degree of freedom analysis for this process. (d) Depending on your results from part (b), do one of these three things: (i) (ii) (iii) If the DOF is negative, show where there is a contradiction or redundancy. If the DOF is zero, determine how much formaldehyde, carbon dioxide, and formic acid is produced. If the DOF is…

Consider the following reaction: 10 KNO3(s) +8 C(s) +3 S(s) 2 K2CO3(s) + 3 K,SO,(s) + 6 CO2(g) + 5 N2(g) you mix 0.75 kg of KNO3 with 0.75 kg of sulfur in the presence of excess carbon and the reaction proceeds with 55% yield, what mass of gas-phase products (i.e., CO2 plus N2) will leave the reaction mixture? Show complete work including all calculations, units, appropriate significant figures, and 1-5 key words of explanation at each step of your calculation. If

Determine the enthalpy of combustion of liquid octane (C8H18) at 25°C and 1 atm, using the enthalpy of formation data from Table A–26. Assume that the water in the products is in the liquid form. Compare your result to the value listed in Table A–27.

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

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).

1. An impure sample of compound A is contaminated with two impurities B and C. The sample is to be purified by recrystallization using ethanol as the solvent. The solubility properties of the three components are summarized below. Solubility in Solubility in ethanol Solubility in 50 mL Solubility in 50 mL ethanol at -78 °C at - 0°C ethanol at -78 °C ethanol at - 0°C (g) (g) Compound A 0.12 g/mL 0.02 g/mL Impurity B 0.58 g/mL 0.04 g/mL Impurity C 0.005 g/mL 0.0003 g/mL The impure (7.5 g) sample contains 5.0 g of compound A, 1.5 g of B and 1.0 g of C and is recrystallized using 50 mL of ethanol. The sample is boiled with 50 mL of ethanol, filtered by gravity and then cooled in ice and filtered by suction. a) How much compound A should be obtained as the final product? Will the sample be contaminated with any of the impurities? Explain (using calculations to support your answer-fill in the missing masses in the table above). Hint: For this question you should calculate the mass of each…

Ethylene oxide (EO) is prepared by the vapor-phase oxidation of ethylene. Its main uses are in the preparation of the antifreeze ethylene glycol and in the production of poly(ethylene terephthalate), which is used to make beverage bottles and fibers. Pure EO vapor can decompose explosively: H,C-CH2(g)-→ CH(g) + C0(g) | Liquid EO has AH = -77.4 kJ/mol and AH ° for its vaporization 569.4 %3D %3D J/g. External heating causes the vapor to decompose at 14.528 bar and 92.4°C in a distillation column. What is the final temperature if 1.932 mols of EO reacted and the average specific heat capacity of the products is 2.769 J/g.°C?