CO(g) + 2 H2(g) ------------ CH3OH(g) Keq = 290
[H2] = 0.080M [CO] = 0.025M
Keq = [CH3OH] / [ CO] [H2[^2
290 = [CH3OH]/ ( 0.025) ( 0.080)^2
[ CH3OH] = 0.0464 M
Concentration of CH3OH = 0.0464 mol/L = 0.0464 M
6. In the presence of a catalyst, methanol, CH,OH, can be prepared by the reaction of...
______________________________________________________________________ Methanol, CH, OH, formerly known as wood alcohol, is manufactured commercially by the following reaction: CO(g) + 2H2 (9) = CH2OH(9) A 1.500 L vessel was filled with 0.1560 mol CO and 0.3070 mol H. When this mixture came to equilibrium at 500 K, the vessel contained 0.1060 mol CO. How many moles of each substance were in the vessel at equilibrium? mol CO mol H2 mol CH3OH An experimenter places the following concentrations of gases in a closed...
A mixture of carbon monoxide, hydrogen, and methanol, CH, OH, is at equilibrium according to the equation CO(g) + 2H2 (9) = CH3OH(9) At 270°C, the mixture is 5.0 x 10-2 M CO.0.760 M H2, and 9.8 x 10-3 M CH3OH What is Ke for this reaction at 270°C? Ke= When 0.125 mol of NO and 18.50 g of bromine are placed in a 1.00-L reaction vessel and sealed, the mixture is heated to 350 K and the following equilibrium...
A) The formaldehyde, CH2O, can be prepared from methanol, using a copper catalyst, according to the following reaction: CH3OH (g) → CH2O (g) + H2 (g) If 25.7 g of CH2O (g) are produced for each mole of methanol that reacts, calculate: to. Theoretical performance b. Real or experimental performance c. Percent of yield Experimental yield and percentage yield values are not given B) A saturated solution of Mg (OH) 2 in contact with solid in solution, is present at...
When methanol, CH, OH, is burned in the presence of oxygen gas, 02, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH, OH(g) + O2(g) → CO2(g) + 2 H2O(1) AH = -764 kJ How much methanol, in grams, must be burned to produce 609 kJ of heat? mass: mass: g
2. We wish to produce formaldehyde by the gas-phase pyrolysis of methanol, CH,OH (8)=CH,0 (8)+H, () The following table provides AH 295, AGM298 and C/R = A+BT +CT2 + DT ?, T'in K, for the species involved in the pyrolysis reaction. Species AH 29(J/mol) AG298 (J/mol) A 10B 10°C 10 D 0 CH,OH CH,0 H -200660 -108570 -161960 -102530 2.211 2.264 3.249 12.216 7.022 0.422 -3.450 -1.877 0 0.083 0 0 0 (a) (15 pts) Calculate heat of reaction and...
Syngas can be burned directly or converted to methanol. Calculate AH for the reaction CO(g) + 2H2 (g) → CH3OH(1) You may need to use the following data: Substance and State AHf (kJ/mol) CO(g) H2(9) CH3OH(l) -110.5 239 △H = kJ
7) Given the following reaction: CO(g) + 2H2(g) = CH,OH(g) In an experiment, 0.57 mol of CO and 0.65 mol of H, were placed in a 1.00-L reaction vessel. At equilibrium there were 0.35 mol of CO remaining. Ke at the temperature of the experiment is a) 17.5 b) 12.7 14.3 d) 0.132 e) None of the above
7) Given the following reaction: CO(g) + 2H2(g) = CH,OH(g) In an experiment, 0.57 mol of CO and 0.65 mol of H, were placed in a 1.00-L reaction vessel. At equilibrium there were 0.35 mol of CO remaining. Ke at the temperature of the experiment is a) 17.5 b) 12.7 14.3 d) 0.132 e) None of the above
Q.2-I completted Parts A,B,C. i need help with part D The synthesis of methanol from carbon monoxide and hydrogen gas is described by the following chemical equation: CO(g) + 2H (8) CH, OH(g) The equilibrium constant for this reaction at 25°C is K -2.3 x 104. In this tutorial, you will use the equilibrium constant expression to find the concentration of methanol at equilibrium, given the concentration of the reactants. Part A Determine the expression for the equilibrium constant, K,...
a) (10 points) The gas phase reaction between methanol (CH,OH) and water that produces carbon dioxide and hydrogen is accompanied by an increase in entropy under standard conditions (AS。-17691/mol). At approximately what temperature does this reaction become spontaneous? 6. (AH for gaseous CH,OH, H20 and CO, are-200.7,-241 8 and-393.5kJ/mol, respectively) b) (10 points) What is the value of the equilibrium constant for the reaction described in part (a) at 25°C?