"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 50 L tank with 18. mol Oof carbon monoxide gas and 23. mol of water vapor. When the mixture has come to equilibrium she determines that it contains 7.0 mol of carbon monoxide gas, 12. mol of water vapor and 11. mol of hydrogen gas. The engineer then adds another 5.0 mol of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the moles of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. |mol

1. The reaction shown below is carried out at various temperatures and the value of Kc determined. Draw particulate representations that show the relative amounts of each reactant and product that would roughly correspond to the value of K. Legend = PC13 = Cl₂ ∞ = = PC15 PC13 (g) + Cl2 (g) = PC15 (g) Magnitude of K Particulate diagram of equilibrium mixture 1 x 10 -3 1 x 105

Decide whether each of the following statements is true or false.  If false, change the wording of the statement to make it true.   a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction.  d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.

Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 50 L tank with 6.5 mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 4.8 mol of nitrogen dioxide gas. The engineer then adds another 3.3 mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. 00. Ar mol x10 Ś ? Explanation © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Check 0: