Question

Home Work Due Next Class Name: For the following reaction in a 5.0 L reaction vessel and at some temperature: CO2(g) + H2(g) CO(g) H20(g) 2. Ke-0.20 at this temperature. Complete the following table (use x where appropriate): CO2 1.00 H2 2.00 со 0 H20 0 initial moles change in moles equilibrium moles equilibrium conc equilibrium conc value (no "r") Verify that your equilibrium concentrations are correct! 3. The following reaction does not proceed at room temperature (the equilibrium constant is exceedingly low, 10-31, but NO is produced at higher temperatures (such as found in automobile engines). N2(g) + 02(g)2 NO(g) Suppose that 5.00 moles of N2 and 10.00 moles of O2 are added to a reaction chamber at room temperature. The temperature is increased to 1000°C. If x moles of Nz react, how many moles of O2 react? How many moles of NO are formed?

Answer 1

Equilibrium constant(K_{​​​​​​c}​​​) is a ratio of concentration of reactants and products at equilibrium.

2. 2. Con- 2-M dissoci 사e moles [CO2] [2) 2 0-4, b=-15 2 q

X is 8-062 2. 883 Valve of x : am not become more than İ , because Some Com Centrafion of Co2 must be Present at the equilibrium x0-867 moles C02 -H CO H20 I-o0 2.00 nitia moles Change iv mole^' M- O.867 2- mole 0.133 moles ST O 867 Conc' mole づ0-133 1.133 0- 867 Vo lume 0.0266 1 0. 2266M 10.1 734M | Ο:/フ3У