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11 Nov 2019
6 Consider the following balanced reaction N2 to, F NO2 with ak,=1.7 10-17 at 25°C a. If 5.37 mol of N2 reacts with 7.82 mol of O2 in a 13.5 L reaction vessel at 25 °C, calculate the equilibrium partial pressures of each molecule b. Convert Kp to Ko c. If the total pressure of the system was increased, would the system need to form more products or reactants to remain at equilibrium? Demonstrate this mathematically. d reaction. He t E~ã-HF , , with a K. = 1 1
6 Consider the following balanced reaction N2 to, F NO2 with ak,=1.7 10-17 at 25°C a. If 5.37 mol of N2 reacts with 7.82 mol of O2 in a 13.5 L reaction vessel at 25 °C, calculate the equilibrium partial pressures of each molecule b. Convert Kp to Ko c. If the total pressure of the system was increased, would the system need to form more products or reactants to remain at equilibrium? Demonstrate this mathematically. d reaction. He t E~ã-HF , , with a K. = 1 1
Bunny GreenfelderLv2
15 Apr 2019