What is the equilibrium partial pressure of methane, PCH4 in the reaction that follows given that...
What is the equilibrium partial pressure of methane, PCH4 in the reaction that follows given that the equilibrium partial pressure of hydrogen, PH2 = 1.22 atm and Kp = 0.262 at 1000 oC? C (s) + 2 H2 (g) -> CH4 (g Answer Choices: 1. PCH4 = 0.320 atm 2. PCH4 = 0.390 atm 3. PCH4 = 0.565 atm 4. PCH4 = 4.66 atm 5. PCH4 = 5.68 atm
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What is the equilibrium partial pressure of methane, PCH4 in the
reaction that follows given that...
Be sure to answer all parts. A) Nitrogen dioxide decomposes according to the reaction 2 NO2(g)...
Be sure to answer all parts. A) Nitrogen dioxide decomposes according to the reaction 2 NO2(g) ⇌ 2 NO(g) + O2(g) where Kp = 4.48 × 10−13 at a certain temperature. If 0.85 atm of NO2 is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO(g) and O2(g)? ___atm O2 ___atm NO B) For the following reaction, Kp = 0.262 at 1000°C: C(s) + 2H2(g) ⇌ CH4(g) At equilibrium, the partial...
The equilibrium constant Kp for the reaction C(s)+H2O(g)⇌CO(g)+H2(g) is 2.44 at 1000 K. What are the...
The equilibrium constant Kp for the reaction C(s)+H2O(g)⇌CO(g)+H2(g) is 2.44 at 1000 K. What are the equilibrium partial pressures of H2O, CO, and H2 if the initial partial pressures are PCO= 1.30 atm, and PH2= 1.40 atm? Part A What is the equilibrium partial pressure of H2O? What is the equilibrium partial pressure of CO? What is the equilibrium partial pressure of CO?
Methane (CH4 ) reacts with hydrogen sulfide (H2S) to yield H2 and carbon disulfide (CS2 ),...
Methane (CH4 ) reacts with hydrogen sulfide (H2S) to yield H2 and carbon disulfide (CS2 ), a solvent used manufacturing rayon and cellophane; CH4 (g) + 2 H2S(g) = CS2 (g) + 4 H2 (g). What is the value of Kp at 1000K if the partial pressure in an equilibrium mixture at 1000K are 0.20atm of CH4 , 0.25 atm of H2S, 0.52 atm of CS2 , and 0.10 atm of H2 .
The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) > CH4(g)...
The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) > CH4(g) + CCl4(g) Calculate the equilibrium partial pressures of all species when CH2Cl2(g) is introduced into an evacuated flask at a pressure of 0.939 atm at 350 K. PCH2Cl2 = atm PCH4 = atm PCCl4 = atm
. Calculate the partial pressure of H2(g) at equilibrium for the following reaction at 90.0°C if...
. Calculate the partial pressure of H2(g) at equilibrium for the following reaction at 90.0°C if the partial pressure of C2H2(g) is 1.8 atm and the partial pressure of C2H6(g) is 0.30 atm. C2H2(g) + 2H2(g) ⇄ C2H6(g) KP = 0.045
KP for the reaction 2HI→I2 +H2 is 10.5 at 25c calculate the equilibrium partial pressure of...
KP for the reaction 2HI→I2 +H2 is 10.5 at 25c calculate the equilibrium partial pressure of HI, I2, and H2 if the initial partial pressure of HI is 4.5 atm
At 6 oC the equilibrium constant for the reaction: 2 HI(g) H2(g) + I2(g) is KP...
At 6 oC the equilibrium constant for the
reaction:
2 HI(g) H2(g) + I2(g)
is KP = 2.66e-11. If the initial pressure of HI is
0.00837 atm, what are the equilibrium partial pressures of HI,
H2, and I2?
We were unable to transcribe this imageAt 6 °C the equilibrium constant for the reaction: 2 HI(g) = H2(g) + 12(g) is Kp = 2.66e-11. If the initial pressure of HI is 0.00837 atm, what are the equilibrium partial pressures of HI,...
A gas phase reaction at equilibrium has the equilibrium expression: (PCS2 ) x (PH2)4 / (PCH4)...
A gas phase reaction at equilibrium has the equilibrium expression: (PCS2 ) x (PH2)4 / (PCH4) x (PH2S)2 What is the reaction equation? A. CH4 + H2S ⇌ CS2 + H2 B. CS2 + 4 H2 ⇌ CH4 +2 H2S C. CH4 + 2 H2S ⇌ CS2 + 4 H2 D. 2 CH4 + H2S ⇌4 CS2 + H2 E. CS2 + CH4 ⇌ H2 + H2S
The reaction C(s)+2H2(g)⇌CH4(g) has Kp=0.263 at 1000. K. Calculate the total pressure at equilibrium when 5.759...
The reaction C(s)+2H2(g)⇌CH4(g) has Kp=0.263 at 1000. K. Calculate the total pressure at equilibrium when 5.759 g of H2 and 22.94 g of C(s) are placed in a 9.88 L flask and heated to 1000. K. Ptotal= ? atm Calculate the total pressure when 5.759 g of H2 and 8.755 g of C(s) are placed in a 9.88 L flask and heated to 1000. K. Ptotal= ? atm
The equilibrium constant for the following reaction is 50.5 at 448 oC. H2(g) + ...
The equilibrium constant for the following reaction is 50.5 at 448 oC. H2(g) + I2(g) ⇌ 2 HI(g) a. Find DGorxn at 448 oC. (This is the change in free energy when the partial pressure of each gas is 1 atm and the T is 448 oC.) b. What is DGrxn when T = 448 oC and PH2 = 1 atm, PI2 = 0.1 atm, PHI = 0.1 atm? c. Is the forward reaction spontaneous...
At 6 oC the equilibrium constant for the
reaction:
2 HI(g) H2(g) + I2(g)
is KP = 2.66e-11. If the initial pressure of HI is
0.00837 atm, what are the equilibrium partial pressures of HI,
H2, and I2?
We were unable to transcribe this imageAt 6 °C the equilibrium constant for the reaction: 2 HI(g) = H2(g) + 12(g) is Kp = 2.66e-11. If the initial pressure of HI is 0.00837 atm, what are the equilibrium partial pressures of HI,...
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