Consider a chemical reaction CO(g)+2H, (g) = CH,OH (g). When 2 moles of CO were reacting...
Consider a chemical reaction CO(g) + 2H, (g) = CH OH(g). When 2 moles of Co were reacting with 4 moles of H, at temperature 500K and pressure p = 100 bar, and chemical equilibrium was reached, n = 0.366 moles of CO was consumed. a) (10 pts) Based on the given data determine the value of the chemical equilibrium constant K(T) for T = 500K. b) (10 pts) Consider now the same reaction, when 3 moles of CO are...
=At 1650°C, the equilibrium constant for the reaction CO(g) + 2H 2 (g) =CH 3 OH(g) has the value K p = 1.4 x 10 –7 . Calculate G° for this reaction at 1650°C.
8.7 was incorrect Consider the following reaction: CH, OH(9) = CO(g) + 2H (9) Part A Calculate AG for this reaction at 25°C under the following conditions PCH,OH-0.850 am Pco 0.145 atm 0 .170 atm P AEP O ? AG-8.7
Ch. 13 NAME 1. Consider the reaction: 2NO (g)+ 2H:(g) N2(g)+ 2H O (g) At a certain temperature, the equilibrium concentrations are [NO]-0.31 M [H2]-0.16 M [N2] 0.082 M and [H:0]-4.64 M (a) Write the equilibrium expression for the reaction. (b) Determine the value of the equilibrium constant 2. The equilibrium constant Kc for the following reaction is 150.7 at 1 15°C: 12 (g) + Br2 (g) ←→ 2 IBr(g) 2.00 moles of each gas (l2, Br: and IBr) are...
20. If K =(0.92) at a (150°C) for the equilibrium reaction: CO(g) + 3H2(g) CH(g) + H2O(g) The K of the reaction is : A) 5.63x 104 B) 2.32 x10+ C) 4.20 x105 D ) 3.29 x 109. Putor (*): 1. Reaction in which entire amount of the reactants is not converted into products is termed as reversible reaction ( ). 2. For exothermic reactions raising the temperature causes a shift to the right (X). 3. If the number of...
In the Lebedev's process 1,3-butadiene is produced from ethanol according to the following chemical equation 20,H,OH(g)->CH.-CH-CH-CH2(g)+2H,O(g)+H2(g) Calculate the butadiene percent yield of the reaction at T-4 lXata 50 K andp 2 atm. CH,OH2348 110.2 -241.8 C4H, H20 167.9 150.7 -228.6
= Objective Knowledge Check Consider the following chemical equilibrium: C(s)+2H, (g) =CH, (g) Now write an equation below that shows how to calculate K, from K for this reaction at an ab room temperature. If you include any common physical constants in your equation be sure you K = 0 X 6 X
Consider the following reaction CO(g) + 2H2(x) = CH2OH(g) The reaction between CO and His carried out at a specific temperature with initial concentrations of CO .025 M and H-0.55 M At equilibrium, the concentration of CH, OH 0.11 M Part A Find the equilibrium constant at this temperature Express your answer using two significant figures. VOAD
10. (5 pts) Consider the following reaction in equilibrium H2(g) + Brz(g) → 2 HBr (g) AH = + 68 kJ How will each of the following changes affect the equilibrium concentrations of each chemical: a) addition of HBr(g) b) increasing temperature c) increasing pressure d) decreasing volume of the reacting vessel at constant temperature. e) addition of bromine f) addition of argon g) addition of catalyst
4. Consider the following reaction: CO(g)+2H2(g) CH,OH(g) A reaction mixture at 780°C initially contains [CO] 1.00M, [Hal-2.00M and [CH3OH-0.00M. At equilibrium, the CO concentration is found to be 0.50M. What is the equilibrium constant for the reaction? (a) 26 (b) 0.385 (c) 4.00 (d) 0.278 (e) 1.00 this table might help Co H2l CH3OH