2.

the gas phase reaction A+B<-->C+D takes place in a batch reactot at 300C. The eq constant k at 300C is 9.0.The reactor is initially charged with 6mol A and 6mol B. What is the extent of the reaction at eq ? What are the mole fractions of each gas ?

Solve correctly please. I know the final answer,but need steps to find it with explanation.

question 3 in imageee

H1

A reaction with an activation energy of 94.8 kJ/mol is carried out at 281. K and 376. K. The reaction rate at 376. K is  a) should be the same as at the other temperature b) approximately 1.338 times faster than at 281. K c) approximately 2.821e+4 times faster than at 281. K d) approximately 6.496e+4 times faster than at 281. K

A8

17. The reaction A+B→C+D is carried out at 80 °C in an isothermal, perfectly stirred tank batch reactor. The reaction rate can be described as second-order, where k=0.058 m³ kmol-¹ min¹¹. At 80 °C, 240 kg of material A (MÃ=60 g mol-¹) and 400 kg of material B (M³=80 g mol-¹) is added into the stirred tank. At this point, the volume of the (liquid) reaction mixture is 0.9 m³. The reaction does not change the volume. How much time is required to reach 95% conversion? batch reactor

a) The new engineer you hired suggests operating the reactor at atmospheric pressure (instead of 300kPa) while keeping the temperature constant (at 800 K) to increase the conversion to product “C”.Would decreasing the pressure increase the conversion? Why?b) Would you consider using an inert gas (such as argon) while keeping the T and the P constant toincrease the conversion? Why?c) Is this reaction endothermic or exothermic? List two benefits of operating the reactor at 800 K?Explain with reactions please

You are carrying out a reaction in the laboratory. You need to convert 1.00 mole of reactant X into products. This reaction shows first-order kinetics, and the reaction mixture has a constant volume of 1.00 L. At 1:00pm, you start the reaction at 25\deg C with 1.00 mole of reactant X. At 2:00pm, you find that 0.70 moles of reactant X remain. You immediately increase the temperature of the reaction mixture to 35\deg C. At 3:00pm, you discover that 0.25 moles of reactant X are still present. You want to be able to finish the reaction by 4:00pm, but you cannot stop the reaction until only 0.01 moles of reactant X remain. You must increase the temperature again. What is the minimum temperature required to complete the reaction by 4:00pm? (Remember, the reaction is complete when only 0.01 moles of X remain.)