Construct a BOD demand curve for a sample that has a first order reaction constant K...

Construct a BOD demand curve for a sample that has a first order reaction constant K of 0.16 day–1 (base 10) and a nitrogenous reaction constant KN 0.08 day–1 (base 10). Nitrification is not significant until a period of 7.5 days has passed. The ultimate first stage BOD is 335 mg/L and the ultimate nitrogenous demand is 120 mg/L. 1) What is the total BOD exerted at 10 days? 2) How many complete days are required to exert at least 90% of the expected demand?

Solutions

Expert Solution

Ally Wells answered 1 year ago

Next > < Previous

Related Solutions

What is the rate constant of a first-order reaction that takes 127 seconds for the reactant...

What is the rate constant of a first-order reaction that takes 127 seconds for the reactant concentration to drop to half of its initial value?

a) A first order reaction is 28.5 % complete in 1908 minutes. Determine the rate constant,...

a) A first order reaction is 28.5 % complete in 1908 minutes. Determine the rate constant, k, for the reaction b) A first order reaction has a of 136.25 minutes. Determine how much time will be required for 39.5% of the original material to decompose. c) It took 62.43 days for 50% of a substance to decompose. If the reaction follows first order kineticsdetermine the value of the rate constant, k in s-1.

The second order reaction 2A2B3 -----> A4B6 has a rate constant, k, of 7.35 x 10-3M-1S-1...

The second order reaction 2A2B3 -----> A4B6 has a rate constant, k, of 7.35 x 10-3M-1S-1 at a certain temperature. If [A2B3]0 = 1.32M, how much time (s) does it take to reduce the concentration to 27% of the original? (please explain) The decomposition of hydrogen peroxide H2O2(l) ---> H2(g) + O2(g) has a rate constant of 1.06 x 10-3min-1. how long (min) will it take for the concentration of H2O2 to decompose by 60%? (please explain) the decomposition of...

The first-order rate constant for the reaction of methyl chloride (CH3Cl) with water to produce methanol...

The first-order rate constant for the reaction of methyl chloride (CH3Cl) with water to produce methanol (CH3OH) and hydrochloric acid (HCl) is 3.32 × 10−10 s−1 at 25°C. Calculate the rate constant at 50.3°C if the activation energy is 116 kJ/mol.

The rate constant for a first order reaction is 0.060s-1. when the temperature is increased from...

The rate constant for a first order reaction is 0.060s-1. when the temperature is increased from 298K to 367 K , the rate constant increases to 0.18s-1. Calculate the activation energy for this reaction. Use kJ/mol for the units. The activation energy in kJ/mol equals (include the units in your answer):

The following reaction is first order in N2O5: N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at...

The following reaction is first order in N2O5: N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. A. Calculate the rate of the reaction when [N2O5]= 5.9×10−2 M. B. What would the rate of the reaction be at the same concentration as in Part A if the reaction were second order? (Assume the same numerical value for the rate constant with the appropriate units.) C. What would the rate of the reaction be at the same...

The following reaction is first order in N2O5: N2O5(g)?NO3(g)+NO2(g) The rate constant for the reaction at...

The following reaction is first order in N2O5: N2O5(g)?NO3(g)+NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. A) Calculate the rate of the reaction when [N2O5]= 5.4

The reaction below has an equilibrium constant K p =2.2× 10 6 at 298 K. 2...

The reaction below has an equilibrium constant K p =2.2× 10 6 at 298 K. 2 COF 2 (g)⇌ CO 2 (g)+ CF 4 (g) Part A Calculate K p for the reaction below. COF 2 (g)⇌ 1 2 CO 2 (g)+ 1 2 CF 4 (g) Part B Calculate K p for the reaction below. 2 3 COF 2 (g)⇌ 1 3 CO 2 (g)+ 1 3 CF 4 (g) Part C Calculate K p for the reaction below....

The equilibrium constant for the reaction below is K = 0.36 at 400 K. If 1.5...

The equilibrium constant for the reaction below is K = 0.36 at 400 K. If 1.5 g of PCl5 was initially placed in a reaction vessel with a volume of 250 cm3, what is the molar concentration of each gas at equilibrium? What is Delta Gorxn for the reaction: PCl5 (g) à PCl3 (g) + Cl2 (g) - Please show all work.

a. A certain first-order reaction (A→products) has a rate constant of 3.00×10−3 s−1 at 45 ∘C....

a. A certain first-order reaction (A→products) has a rate constant of 3.00×10−3 s−1 at 45 ∘C. How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25% of the original concentration? b. A certain second-order reaction (B→products) has a rate constant of 1.85×10−3M−1⋅s−1 at 27 ∘C and an initial half-life of 300 s . What is the concentration of the reactant B after one half-life?

Subjects