The equilibrium constant for the reaction CCl4(g) = C(s) + 2Cl2(g) at 700ºC is 0.85. Determine the...

The equilibrium constant for the reaction CCl4(g) = C(s) + 2Cl2(g)

at 700ºC is 0.85. Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 2.30 atm at 700ºC.

Expert Solution

queen_honey_blossom answered 1 week ago

The equilibrum constant Kc is 0.01323 for the reaction: CCl4 (g) <----> C(s) + 2 Cl2...

The equilibrum constant Kc is 0.01323 for the reaction: CCl4 (g) <----> C(s) + 2 Cl2 (g) At 300k a 5L flask originally contained 0.0828M of CCl4, 0.0444 M of C and 0.0546M of Cl2. Determine the concentration of Cl2 when equilibrium is reached.

Write the equilibrium constant for the following reaction: 2Cl2 + 2H2O <---> 4HCL + O2

The equilibrium constant KP for CCl4(g) f15g2a33g1.jpgC(s) + 2 Cl2(g) is 0.76 at 700 K. What...

The equilibrium constant KP for CCl4(g) f15g2a33g1.jpgC(s) + 2 Cl2(g) is 0.76 at 700 K. What percentage (%) of CCl4 is converted into C and Cl2 when a flask charged with 3.00 atm of CCl4 reaches equilibrium at 700 K?

At 100.0 C, the equilibrium constant for the reaction: CO (g) + Cl2 (g) <--> COCl2...

At 100.0 C, the equilibrium constant for the reaction: CO (g) + Cl2 (g) <--> COCl2 (g) has a value of 4.6 x 109. If 0.40 mol of COCl2 is placed into a 10.0 L flask at 100.0 C, what will be the equilibrium concentration of all species? (A simplifying approximation that will make the solution of the resulting equation easier is to note that x is much less than 0.040mol/L. This means that 0.040 -x is approximately 0.040.)

Calculate ΔrH for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) Use the following reactions and given ΔrH's. C(s)+2H2(g)→CH4(g)ΔrH=−74.6kJmol−1C(s)+2Cl2(g)→CCl4(g)ΔrH=−95.7kJmol−1H2(g)+Cl2(g)→2HCl(g)ΔrH=−92.3kJmol−1

Calculate ΔrH for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) Use the following reactions and given ΔrH's. C(s)+2H2(g)→CH4(g)ΔrH=−74.6kJmol−1C(s)+2Cl2(g)→CCl4(g)ΔrH=−95.7kJmol−1H2(g)+Cl2(g)→2HCl(g)ΔrH=−92.3kJmol−1

Calculate ΔrH for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) Use the following reactions and given ΔrH's. C(s)+2H2(g)→CH4(g)ΔrH=−74.6kJmol−1C(s)+2Cl2(g)→CCl4(g)ΔrH=−95.7kJmol−1H2(g)+Cl2(g)→2HCl(g)ΔrH=−92.3kJmol−1

Calculate ΔrH for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) Use the following reactions and given ΔrH's. C(s)+2H2(g)→CH4(g)ΔrH=−74.6kJmol−1C(s)+2Cl2(g)→CCl4(g)ΔrH=−95.7kJmol−1H2(g)+Cl2(g)→2HCl(g)ΔrH=−92.3kJmol−1

Express the equilibrium constant for the following reaction. 5P4O10(s) ⇋ 5P4(s) + 25O2(g)

Express the equilibrium constant for the following reaction. P4(s)+5O2(g)<>P4O10(s)

(a) For the reaction 2 A(aq) ⇋ 2 B(g) + C(g), the equilibrium constant is 4.59...

(a) For the reaction 2 A(aq) ⇋ 2 B(g) + C(g), the equilibrium constant is 4.59 at 25.0oC. If the concentrations of B(aq) and C(aq) are each 0.311 M, what concentration of A(aq) is required to have a ΔG value of -6.66 kJ/mol? The temperature is 25.0oC. (b) We have a buffer solution that was produced by adding 11.9 g of NaOH to 2.000 L of a 0.666 M solution of HA(aq). The pH of the buffer solution is 3.25...

The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g) + HF(g) NH4F(s) at...

The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g) + HF(g) NH4F(s) at 25 °C is 10.2. (a) If the partial pressure of ammonia is PNH3 = 0.553 atm (at equilibrium) and solid ammonium fluoride is present, what is the equilibrium partial pressure in atm of hydrogen fluoride at 25 °C? An excess of solid NH4F is added to a container filled with NH3 at 25 °C and a pressure of 1.09 atm. Calculate the pressures of...

Question

The equilibrium constant for the reaction CCl4(g) = C(s) + 2Cl2(g) at 700ºC is 0.85. Determine the...

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Expert Solution

Related Solutions

The equilibrum constant Kc is 0.01323 for the reaction: CCl4 (g) <----> C(s) + 2 Cl2...

Write the equilibrium constant for the following reaction: 2Cl2 + 2H2O <---> 4HCL + O2

The equilibrium constant KP for CCl4(g) f15g2a33g1.jpgC(s) + 2 Cl2(g) is 0.76 at 700 K. What...

At 100.0 C, the equilibrium constant for the reaction: CO (g) + Cl2 (g) <--> COCl2...

Calculate ΔrH for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) Use the following reactions and given ΔrH's. C(s)+2H2(g)→CH4(g)ΔrH=−74.6kJmol−1C(s)+2Cl2(g)→CCl4(g)ΔrH=−95.7kJmol−1H2(g)+Cl2(g)→2HCl(g)ΔrH=−92.3kJmol−1

Calculate ΔrH for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) Use the following reactions and given ΔrH's. C(s)+2H2(g)→CH4(g)ΔrH=−74.6kJmol−1C(s)+2Cl2(g)→CCl4(g)ΔrH=−95.7kJmol−1H2(g)+Cl2(g)→2HCl(g)ΔrH=−92.3kJmol−1

Express the equilibrium constant for the following reaction. 5P4O10(s) ⇋ 5P4(s) + 25O2(g)

Express the equilibrium constant for the following reaction. P4(s)+5O2(g)<>P4O10(s)

(a) For the reaction 2 A(aq) ⇋ 2 B(g) + C(g), the equilibrium constant is 4.59...

The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g) + HF(g) NH4F(s) at...