At 380 0C, the equilibrium concentrations are [CH3OH] = 0.20 M, [CO] = 0.35 M, and [H2] = 2.1 M for the reaction: CH3OH (g) ↔ CO (g) + 2H2 (g) Calculate K at this temperature
The answer is K=7.7. Please show all steps. Thank You in advanced.
At 380 0C, the equilibrium concentrations are [CH3OH] = 0.20 M, [CO] = 0.35 M, and...
if K=0.60 for the reaction CO(g)+2H2(g) <—> CH3OH(g), what is [CH3OH] if [CO]=[H2]=0.35 M
1-The equilibrium constant Kc for the equation 2H2(g) + CO(g) ⇌ CH3OH(g) is 11 at a certain temperature. If there are 2.63 × 10−2 moles of H2 and 7.15 × 10−3 moles of CH3OH at equilibrium in a 6.29−L flask, what is the concentration of CO? ?M 2-In an analysis of the following reaction at 100°C,Br2(g) + Cl2(g) ⇌ 2BrCl(g) the equilibrium concentrations of the reactants were found to be [Br2] = 4.0×10−3M and [Cl2] = 7.7 ×10−3M. The equilibrium...
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) The reaction between CO and H2 is carried out at a specific temperature with initial concentrations of CO = 0.26 M and H2 = 0.52 M. At equilibrium, the concentration of CH3OH is 0.11 M. Find the equilibrium constant at this temperature
The reaction between CO and H2 is carried out at a different temperature with initial concentrations of [CO] = 0.31 M and [H2]= 1.4 M . CO(g)+2H2(g)⇌CH3OH(g) At equilibrium, the concentration of CH3OH is 0.09 M Find the equilibrium constant at this temperature.
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) This reaction is carried out at a specific temperature with initial concentrations of [CO] = 0.27 M and [H2]= 0.49 M. At equilibrium, the concentration of CH3OH is 0.11 M. Find the equilibrium constant at this temperature. Express the equilibrium constant to two significant figures.
Consider the reaction: CO(g)+2H2(g)⇌CH3OH(g) An equilibrium mixture of this reaction at a certain temperature was found to have [CO]= 0.115 M , [H2]= 0.124 M , and [CH3OH]= 0.235 M . Part A What is the value of the equilibrium constant at this temperature?
part b Part Suppose that the molar concentrations for CO and H, at equilibrium are (CO) = 0.03 M and H2) = 0.06 M. Use the formula you found in Part B to calculate the concentration of CH, OH. Express your answer to one decimal place and include the appropriate units. View Available Hint(s) : HÅR O a ? (CH3OH) = Value Units Submit art D Complete previous part(s) Review Constants I Periodic Table The equilibrium-constant expression is a mathematical...
Consider the reaction CO(g) + 2H2(g) = CH3OH(g) An equilibrium mixture of this reaction at a certain temperature was found to have [CO] = 0.125 M, [H2] = 0.124 M, and (CH3OH) = 0.275 M. Part A What is the value of the equilibrium constant at this temperature? Express the equilibrium constant to three significant figures. IVO AE ? Keq = 181 Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining
CO(g)+2H2(g)⇌CH3OH(g)CO(g)+2H2(g)⇌CH3OH(g) The reaction between COCO and H2H2 is carried out at a specific temperature with initial concentrations of COCO = 0.30 M M and H2H2 = 0.52 M M. At equilibrium, the concentration of CH3OHCH3OH is 0.16 M M.
Consider the reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.25 −L flask at 500 K contains 9.02 g CO and 0.57 g of H2. At equilibrium, the flask contains 2.34 g CH3OH. Calculate the equilibrium constant at this temperature.