An evacuated reaction vessel is filled with 0.800 atm of N₂ and 1.681 atm of Br2. When equilibrium is established according to the reaction below, there are 1.425 atm of Br2 remaining in the vessel. What is the equilibrium partial pressure of NBr3? 2 NBr3 (g) = N₂ (g) + 3 Br2 (g)

Suppose a  500.mL  flask is filled with  1.0mol  of  Cl2 ,  1.3mol  of  CHCl3  and  0.50mol  of  CCl4 . The following reaction becomes possible: +Cl2gCHCl3g    +HClgCCl4g The equilibrium constant  K  for this reaction is  1.32  at the temperature of the flask. Calculate the equilibrium molarity of  CHCl3 . Round your answer to two decimal places.

When 3.00 mol of A and 1.00 mol of B are mixed in a 1.00 L vessel, the following reaction takes place: A(g) + B(g) →2 C(g). The equilibrium mixture contains 0.50 mol of C. What is the value of the equilibrium constant for the reaction? 0.24 8.3 O 0.20 0.12

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 500. mL flask with 0.82 atm of carbon monoxide gas and 0.85 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.33 atm of carbon monoxide gas, 0.36 atm of water vapor and 0.49 atm of hydrogen gas. The engineer then adds another 0.41 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. atm