The rate constant for the reaction NO₂(g) + O3(g) → NO3(g) + O₂(g) was determined over a temperature range of 40 K, with the following results: T (K) 203 213 223 233 243 k (M¹s¹) 4.14 X 105 7.30 X 105 1.22 X 106 1.96 X 106 3.02 X 106 a. Determine the activation energy for the reaction. b. Calculate the rate constant of the reaction at 300 K.

The growth of baker's yeast (Saccharomyces cerevisiae) on glucose under anaerobic conditions can be described by the following equation:C6H12O6 + β NH3 → 0.59 CH1.74N0.2O0.45 + 0.43 C3H8O3 + 1.54 CO2 + 1.3 C2H5OH + 0.036 H2O a) Determine the value of the biomass yield coefficient YX/Sb) Determine the values of the yield coefficients in products YEtOH/S and Yglycerol/Sc) Calculate the value of the coefficient β

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

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

How many electrons are transferred in the following process, given the unbalanced reaction? PbO2 (s) + H* (aq) + Fe (s) → Fe3+(aq) + Pb2+ (aq) + H20 (1) Group of answer choices A-1 В-2 C-6 D-4 Е-3

The equilibrium constant, K., for the following reaction is 9.52×10-2 at 350 K. CH4 (g) + CC14 (g) =2 CH2Cl2 (g) Calculate the equilibrium concentrations of reactants and product when 0.277 moles of CH, and 0.277 moles of CCl, are introduced into a 1.00 L vessel at 350 K. [ CH4] M [CC4] M [ CH2C1, ] = M

Part a plz!

Nitromethane, CH3NO2 , can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainlyCH3NO2(l) + O2(g) → CO2(g) + N2(g) + H2O(g)a. The standard enthalpy change of reaction (ΔH°van ) for the balanced reaction (with lowest whole-number coefficients) is −1288.5 kJ. Calculate ΔHf0 for nitromethane.b. A 15.0-L flask containing a sample of nitromethane is filled with O2 and the flask is heated to 100.°C. At this temperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 950. torr. If the mole fraction of nitrogen (χnitrogen) is 0.134 after the reaction is complete, what mass of nitrogen was produced?

Q3 in image