QUESTION 8 Regarding the following reaction CO₂ (g)+H2 (g)→→CO(g)+H₂O (g) ArH=-41.2kJ/mol Using Le Chatelier's principle to predict (a) to which direction the equilibrium shifts when pressure is decreased. Enter R for reactants, P for products and N for Neither: Direction= ; (b) to which direction the equilibrium shifts when temperature is reduced. Enter R for reactants, P for products and N for Neither: Direction=

Solve please,typed ans need. And need both parts solution,plz don't reject ques. I will rate your answer if correct

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).

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…

Consider the following reaction in a sealed vessel kept at constant temperature: A(g)  ⇌  2B(g) If the reaction is started with 2.0 mol of A and no B, the amount of B at equilibrium is 3.0 mol. How many moles of A should one start with to obtain 6.0 mol of B at equilibrium under the same conditions (same vessel, same temperature, no gas B present initially)?   A.  5.6 mol   B.  5.0 mol   C.  4.0 mol   D.  6.0 mol   E.  6.5 mol

Now, let's use what we know about chemistry to infer how much acetic acid was in our sample. Let's look closely at the equation for the reaction we performed. HC2H3O2(aq) + NaHCO3(s) → NaC2H3O2(aq) + H2O(1) + CO2(g) Based on this balanced chemical reaction, we can see that for every one mole of CO2 that was produced one mole of acetic acid was consumed. Based on this, calculate the moles of acetic acid and grams of acetic acid that must have reacted in each sample. Sample Data for Vinegar Lab moles CO2 Produced Moles HC2H3O2 Consumed g HC2H302 Consumed by by Reaction by Reaction Reaction -2 g NaHCO3 0.0329 -4 g NaHCO3 0.0464 -6 g NaHCO3 0.0523 -8 g NaHCOз 0.0477 -10 g NaHCO3 0.0489

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?

A student determines the value of the equilibrium constant to be 1.98×10-5 for the following reaction.CO2(g) + H2(g)CO(g) + H2O(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank 1 than zero.Calculate the free energy change for the reaction of 1.74 moles of CO2(g) at standard conditions at 298K.     G°rxn =  kJ

A batch process is operated with the following sequence. The feed to the batch process consists of a solution of 500 L of ethanol with 120 mole of A and 120 mole of B. If the temperature of the solution is sufficient, A and B will react to form P (the desired product): A (eth) + B (eth) → P (s) DHreact  = − 250 kJ/mol (1)  product P is sparingly soluble in ethanol, which helps facilitate its removal from the reaction solution. It can be assumed that the reaction rate is first-order in both the concentration of A (cA ) and B (cB ), and so second-order overall: -r A = k c A cB  (2) The batch process consists of the following FOUR steps: Initially, the tank is empty. 1. Fill tank with solution (ethanol/A/B). 50°C (1 hour) Increase temperature of the feed from 20°C to 2. Reaction takes place isothermally at 50°C (4 hours, to give conversion of 50%) 3. Filtration of reaction solution to give product P (2 hours) 4. Drying with hot nitrogen gas followed by the removal of powder product (3…