I use the equation Kp=Kc(RT)^change in n. I plug in Kp=(.0415)(.08206)(629.15)^1= 2.1425.Borek said:Show how you arrive at the wrong answer then.
In chemistry, equilibrium refers to a state in which the forward and reverse reactions occur at equal rates, resulting in no net change in the concentrations of reactants and products.
According to Le Chatelier's principle, an increase in temperature will favor the endothermic reaction, while a decrease in temperature will favor the exothermic reaction. This means that equilibrium will shift in the direction that consumes or produces heat in order to maintain a constant temperature.
In equilibrium, the partial pressures of each gas involved can be calculated using the ideal gas law, where P is the partial pressure, n is the number of moles, V is the volume, and T is the temperature: P = nRT/V. The total pressure in the system is equal to the sum of all the partial pressures.
The equilibrium constant, K, is determined by taking the ratio of the concentrations of products to reactants at equilibrium, with each concentration raised to the power of its coefficient in the balanced chemical equation. The value of K indicates the extent to which the reaction favors products or reactants at equilibrium.
According to Le Chatelier's principle, an increase in pressure will shift equilibrium in the direction that decreases the total number of moles of gas, while a decrease in pressure will shift equilibrium in the direction that increases the total number of moles of gas. This means that equilibrium will shift to the side with fewer moles of gas in order to relieve the pressure change.