At 1500 °C, Kc = 5.67 for the reaction CH4(g) + H2O(g) CO(g) + 3H2(g) Calculated value of ΔG°1773 for the reaction at this temperature. side note: -25.6 kJ is the wrong answer
Given T = 1500°C = 1773.15 K
And Kc = 5.67
So, ∆G° ( 1500 ) = - 2.303 RT log Kc
So ∆G° = - ( 2.303 x 8.314 x 1773.15 ) log 5.67
∆G° = - 25584.71 J / mol = -25.58 kJ /mol
At 1500 °C, Kc = 5.67 for the reaction CH4(g) + H2O(g) CO(g) + 3H2(g) Calculated...
QUESTION 9 The reaction CO(g) + 3H2(g) + H2O(g) + CH4(e) has a kc - 190 at 727°C. What is the Kp for this reaction? 0.0534 0.0463 0.0382 0.00275 0.0282
For the reaction CH4(g) + H2O(g)3H2(g) + CO(g) H° = 206.1 kJ and S° = 214.7 J/K The equilibrium constant for this reaction at 264.0 K is Assume that H° and S° are independent of temperature.
QUESTION 7 Consider the reaction below. CO(g) + 3H2 (g) CH4(g) + H2O(g) Kc 138 at 1200 K 0.2 mol of CO and 0.3 mol of H2 gas are initially placed in a 1.0 L container. Letting X -concentration of CO reacted leads to the following equilibrium expression. (0.2-x)(0.3-3x) Solving for X gives the following roots x = 0.209045 x-0.107165 +0.0316478 x-0.107165-0.03 16478/ x0.0766248 What is the equilibrium concentration of CH4 in molar? QUESTION 8 Click Save and Submit to...
CH4(g) + H2O(g) >>> CO(g) + 3H2(g) A 200. L reaction vessel containing methane (CH4) at 480K has a pressure of 1.81 atm. 16.2 moles of steam are introduced, and the reaction above takes place. What is the partial pressure of each of the four gases in this balanced equation after the reaction runs to completion? Assume that both volume and temperature remain constant.
5.8 Express K for the reaction CO(g) + 3H2(g) = CH4(g) + H2O(g) in terms of the equilibrium extent of reaction when one mole of CO is mixed with one mole of hydrogen.
5.8 Express K for the reaction CO(g) + 3H2(g) = CH4(g) + H2O(g) in terms of the equilibrium extent of reaction & when one mole of CO is mixed with one mole of hydrogen.
5.8 Express K for the reaction CO(g) + 3H2(g) = CH4(g) + H2O(g) in terms of the equilibrium extent of reaction & when one mole of CO is mixed with one mole of hydrogen.
Consider the reaction CH4(g) + H2O(g)CO(g) + 3H2(g) for which H° = 206.1 kJ and S° = 214.7 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 2.262 moles of CH4(g) react under standard conditions at 298.15 K. Suniverse = J/K (2) Is this reaction reactant or product favored under standard conditions? _________reactantproduct (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is...
For the reaction CH_(g) + H2O(g) +3H2(g) + CO(g) AH° = 206.1 kJ and AS° = 214.7 J/K The standard free energy change for the reaction of 1.73 moles of CH4(9) at 317 K, 1 atm would be kJ. This reaction is (reactant, product) favored under standard conditions at 317 K. Assume that AHⓇ and A Sº are independent of temperature. Submit Answer Retry Entire Group 9 more group attempts remaining For the reaction CH4(g) + H206) CH3CH2OH() AGⓇ =...
Consider the reaction CO(g) + 3H2(g)CH4(g) + H2O(g) Using the standard thermodynamic data in the tables linked above, calculate G for this reaction at 298.15K if the pressure of each gas is 17.11 mm Hg.