Ethylene oxide (C2H4O) is made by the catalytic reaction between ethylene (C2H4) and oxygen.Fresh ethylene, pure oxygen, and recycled ethylene are mixed to give a reactor feed gas containing 55%C2H4 which enters the reactor at 1 atm absolute and 300 oC. From test experiments, the single-pass conversion of ethylene in the reactor is 54% and, of this, 72% goes to ethylene oxide and the balance decomposes to CO2 and H2O. Most of the unreacted ethylene is separated from the reactor exit stream and is recycled, a pure ethylene oxide product stream is produced, and the remaining materials leave in a waste stream which analyses 9.0% ethylene. The production rate of ethylene oxide is 26,430 kg/day.Determine: a) the molar flow rate of fresh ethylene feed; b) the flow rate of the recycle stream; c) the fraction of feed oxygen wasted; and d) the percent excess oxygen

Using data from the table below, estimate the percentage of chlorocyclohexane molecules that have their substituents in an axial orientation at room temperature.

Table 4.1 - http://imgur.com/ZLsHz5S,9ose7I0

Figure 4.12 - http://imgur.com/ZLsHz5S,9ose7I0#1

Find the pH of a 0.170M HClO2(aq) solution. For HClO2, Ka=0.011.

Which of the following electronic transitions in a hydrogen atom will be accompanied by the absorption of electromagnetic radiation of the longest wavelength?

Group of answer choices

A. n = 3 → n = 4

B. n = 6 → n = 5

C. n = 3 → n = 2

D. n = 1 → n = 2

E. n = 4 → n = 5

Determine the pH of a solution that is 3.55% KOH by mass. Assume that the solution has density of 1.01 g/mL.

In each of the following balanced oxidation-reduction equations, identify those elements that undergo changes in oxidation number and indicate the magnitude of the change in each case.

2MnO4−(aq)+3S2−(aq)+4H2O(l)→3S(s)+2MnO2(s)+8OH−(aq)   

4H2O2(aq)+Cl2O7(g)+2OH−(aq)→2ClO2−(aq)+5H2O(l)+4O2(g)

Ba2+(aq)+2OH−(aq)+H2O2(aq)+2ClO2(aq)→Ba(ClO2)2(s)+2H2O(l)+O2(g)

In chemical reactions, heat is converted into chemical energy (the potential energy stored in chemical bonds) or vice versa. Bond energy is the energy required to break one mole of the bond in the gas phase. Since it takes energy to break a bond, bond energies are always positive. Conversely, energy is released when bonds are formed. Thus, the enthalpy change for a reaction can be approximated from ΔHrxn=∑(ΔHbreaking)+∑(ΔHforming) where H represents bond energies for the breaking (positive bond energy) or forming (negative bond energy) of a bond and Hrxn represents the overall enthalpy for the reaction. Use the table to answer questions about bond energies. Bond Bond energy (kJ/mol )

C−C 347

C=C 611

C−H 414

C−O 360

C=OinCO2 799

O−O 142

O=O 498

H−O 464

Calculate the bond energy per mole for breaking all the bonds in methane, CH4. Express your answer to four significant figures and include the appropriate units.

Calculate the bond energy per mole for breaking all the bonds of oxygen, O2? Express your answer to three significant figures and include the appropriate units.

Calculate the bond energy per mole for forming all the bonds of water molecules, H2O. Express your answer to three significant figures and include the appropriate units.

Calculate the bond energy per mole for forming all the bonds of carbon dioxide, CO2. Express your answer to four significant figures and include the appropriate units. ΔHCO2 =

Describe the stage of polymerization through which a phenolic resin passes to become thermoset.

give the structure corresponding to the name (s)-4-chloro-2-pentyne

derive butler-volmer equation from Arrhenius equation

please show all steps

Calculate ΔHrxn for the following reaction:

CaO(s)+CO2(g)→CaCO3(s)

Use the following reactions and given ΔH values: Ca(s)+CO2(g)+12O2(g)→CaCO3(s), ΔH= -812.8 kJ

2Ca(s)+O2(g)→2CaO(s), ΔH= -1269.8 kJ

Express your answer using four significant figures.

what is the degree of polymerization (DP) of LDPE having an average molecular weight (mass) of 27,980?

Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When 0.107 g of Zn(s) is combined with enough HCl to make 54.9 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.0 ∘C to 24.0 ∘C.

Find ΔHrxn for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4.18 J/g⋅∘C as the specific heat capacity.)

Calculate the pH of the following solutions.

A.) 0.36 M NH4NO3

B)0.50 M Ca(NO3)2

C.)0.080 M C6H5NH2

D.) 0.45 M KNO2

5. Suggest 5 ways that the concentration of PH₃ could be increased in the following reaction.

P_{4 (g)} + 6 H_{2 (g)} ⇌ 4 PH_{3 (g)}        ΔH^o = 110 kJ/mol

6. Gaseous nitrogen dioxide forms gaseous dinitrogen tetroxide with a k_eq = 164 at 25°C in a 2.00L container

            a. Write and balance the equation

b. If at a given timepoint the concentrations of nitrogen dioxide was measured to be 0.500 M and the concentration of dinitrogen tetroxide was measured to be 1.25 M, is the reaction at equilibrium?

            c. What are the concentrations at equilibrium?

d. After the initial equilibrium, if 5.00mol of dinitrogen tetroxide was introduced into the container, what are the concentrations of both species when equilibrium reestablishes?