The synthesis of chemical intermediate C can be written as: A + 2 B = 2 C The reaction is to be conducted from a 800 mol/hours feed of reactants containing A and B in a 1/3 mol ratio.  In the process, the yield of C with respect of A reacted is 100% . What is the excess reactant? What is the percentage excess?

) Calculate the equilibrium conversion and concentrations for the following liquid phase reaction: 2A + B ki k-1 C + 2D Ke = 2.93 a) Construct the stoichiometric table. b) Derive the concentrations in terms of conversion of the limiting reactant. c) Derive the equation to solve for the equilibrium conversion of the limiting reactant and calculate the concentration of each substance. Additional data: CAO = 16 mole/L, CBO = 4.8 mole/L, CDo-24 mole/L

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(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction Cl₂(g) + 2e →→→→2Cl¯(aq) Mg(s) Mg2+ (aq) + 2e¯ identification oxidation reduction (2) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients. + +

2. For the combustion of ethanol with air, the reaction proceeds according to the unbalanced reaction below: C₂H6O + O₂ => CO₂ + H₂O An air stream is fed to a reactor to provide oxygen. The reactor operates at steady state, and all reactants and products are gaseous phase. All left over reactants and created products leave the reactor in a single stream. The oxygen is supplied in excess by 10%, and the fractional conversion of the ethanol is 75%. Calculate the mole fraction of ethanol in the outlet stream.

If you feed 10.0g of N2 gas and 10.0g of H2 into a reactor to make ammonia (NH3):a. What is the limiting reactant and the excess reactant?b. What is the maximum number of grams of NH3 that can be produced if 100% of the limiting reactant was reacted?c. If 5.0g of the limiting reactant actually react, what is the fractional conversion of the limiting reactant, and why would you want to make ammonia, what is it useful for?

Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: Cu2+(aq) + 2Ag(s)  Cu(s) + 2Ag+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.  Equilibrium constant: ____ G° for this reaction would be _________greater/ less  than zero.

What is the composition of the final product? Yacetic acid: 0.516 Ymethylacetate: i 0.0179 Ymethanol: 0.233 Ywater: 0.233 c. Suppose it were important to reduce the concentration of methanol by making its conversion at equilibrium 98.5%. Again, assuming the feed to the reactor contains only methanol and acetic acid and that it is desired to produce 65.0 moles of methyl acetate, determine the extent of reaction and moles of methanol and acetic acid that must be fed to the reactor. Extent: 65 Required methanol: 65.98 mol Required acetic acid: i 1459.5 mol

The reaction between nitric oxide and bromine is described by the following chemical equation: 2NO (g) + Br, (g) → 2NOB1 (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: NO (g) +Br, (g) → NOB1, (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism. ローロ

The equilibrium constant, Ke, for the following reaction is 1.80×10-² at 698 K. 2HI(g) H2(g) + I,(g) Calculate the equilibrium concentrations of reactant and products when 0.294 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] M [H2] M [IL] M