a 1l flask is charged with a mixture 0.200 mol NOBr, 0.20 mol Br2 and 0.40 mol NO and warmed up to 50c. when the reaction has come to equilibrium, the flask is found to contain 0.166 mol NOBr. based on these results, what is the value of Kc for this reaction under these conditions?

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Hubert KochLv2

22 May 2020

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An evacuated 1.000 L flask was filled at room temperature with 4.920E-2 mol NO (nitrogen monoxide) and 7.74E-3 mol Br₂ (bromine). The temperature was then raised to 50.5Â°C, and these substances reacted to give nitrosyl bromide, NOBr:

2NO(g) + Br(g) <--> 2NOBr(g)

When equilibrium was achieved, the pressure of the gases in the flask was found to be 1.315 atm.

(a) What was the total moles of gases in the flask at equilibrium?	n_total = mol
(b) How many moles of nitrosyl bromide were formed? What was the moles of each substance in the flask at equilibrium?	n(NO) = mol n(Br₂) = mol n(NOBr) = mol
(c) What are the partial pressures of the different gases in this equilibrium mixture?	p(NO) = atm p(Br₂) = atm p(NOBr) = atm
(d) What is K_p at this temperature?	K_p =

A sample of nitrosyl bromide (NOBr) decomposes according to the equation

2 NOBr(g) 2 NO(g) + Br₂(g)

An equilibrium mixture in a 5.00-L vessel at 100 °C contains 3.22 g of NOBr, 3.08 g of NO, and 4.19 g of Br₂. (a) Calculate K_c. (b) What is the total pressure exerted by the mixture of gases? (c) What was the mass of the original sample of NOBr?

The equilibrium concentration of all components is

The value of K_c for this reaction is

b) Assuming the ideal gas behavior, the total gas pressure corresponds to the partial pressures of each gas in the equilibrium mixture. The number of moles of three gases should be summed, and included in the ideal gas law equation to obtain the total pressure.

The total number of moles of gas is: 0.158 mol. The total pressure is

c) According to the Law of conservation of mass, the mass at the beginning and the mass at the end of reaction must be the same. The total mass at the equilibrium is 3.22 + 3.08 + 4.19 = 10.49 g. The mass of an original sample of NOBr was 10.49 g.