QUESTION 9 The reaction CO(g) + 3H2(g) + H2O(g) + CH4(e) has a kc - 190...

Question

Question

Answer 1

Answer #1

He Olgo + CH419 Rez 190 T=10ook Colgs + 3H2 18) - ang = 2 -(1+3) Kp = kc (RT) Ang = 190 x(0.0821 X 1000)-& Rp = 190 82:1X82-1

Answer 2

Similar Homework Help Questions

At 1500 °C, Kc = 5.67 for the reaction CH4(g) + H2O(g) CO(g) + 3H2(g) Calculated...

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
QUESTION 7 Consider the reaction below. CO(g) + 3H2 (g) CH4(g) + H2O(g) Kc 138 at...

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...

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...

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...

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...

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.

For the reaction CH4(g) + H2O(g)3H2(g) + CO(g) H° = 206.1 kJ and S° = 214.7...

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.
Consider the reaction CO(g) + 3H2(g)CH4(g) + H2O(g) Using the standard thermodynamic data in the tables...

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.
CH4(g) + H2O(g) <-- CO(g) + 3H2(g) Calculate the DG° of a mixture that has initial...

CH4(g) + H2O(g) <-- CO(g) + 3H2(g) Calculate the DG° of a mixture that has initial partial preassures of PCH4 = 1 bar; PH2O = 0.5 bar; PCO=1 bar; PH2 = 1 bar.

Ch4 (g) + H2O (g) -> CO (g) + 3H2 (g) what are the molar masses...

Ch4 (g) + H2O (g) -> CO (g) + 3H2 (g) what are the molar masses for each chemical bond? I was given initial mass of 995g Ch4 and 2510g H2O. what are the rest of the initial masses? what are the initial moles, final moles, and final masses of each chemical bond. also what is the theoretical yield, experimental ratio, and limiting reagent?