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

Expert Solution

queen_honey_blossom answered 2 years ago

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

1)Express the equilibrium constant for the following reaction. 20CH3Br (g) + 10Br2 (g) ⟺ 20CH2Br2 (g)...

1)Express the equilibrium constant for the following reaction. 20CH3Br (g) + 10Br2 (g) ⟺ 20CH2Br2 (g) + 10H2 (g) 2)Find each in equilibrium constant expressions: *6H2(g)+P4(g)⇌4PH3(g) *CO(g)+Cl2(g)⇌COCl2(g) 3)Identify the change that will always shift the equilibrium to the right. 2SO2 (g) + O2 (g) ⇋ 2SO3 (g) a)remove reactant b)adding He c)add Cu d)remove product e)increase the volume

Express the equilibrium constant for the following reaction. 10PCl5(g) ↔ 10PCl3(g) + 10Cl2(g)

Given the following information, answer these questions. P4(g) + 5 O2(g) → P4O10(s) ΔG⁰298 = −2748...

Given the following information, answer these questions. P4(g) + 5 O2(g) → P4O10(s) ΔG⁰298 = −2748 kJ/mol2 H2(g) + O2(g) → 2 H2O(l) ΔG⁰298 = −474.2 kJ/molP4O10(s) + 6 H2O(l) → 4 H3PO4(l) ΔG⁰298 = −349 kJ/mol (a) Determine the standard free energy of formation, ΔG⁰f (in kJ/mol), for phosphoric acid from this information.(Assume that ΔG⁰298 for all elemental substances is negligible.) _______ kJ/mol (b) How does your calculated result compare to the value in the Standard State Thermodynamic Data...

Consider the following reaction: P4(s) + 6F2(g) ----> 4PF3(g) A, 55.0g of P4 were mixed with...

Consider the following reaction: P4(s) + 6F2(g) ----> 4PF3(g) A, 55.0g of P4 were mixed with 32.6g of G2 to produce PF3. Which reaction was the limiting reagent? Explain. B. How many moles of PF3 were produced i the reaction went to completion? C. How many grams of PF3 were collected if the reaction had 85.4% yield

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...

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.

A.) The equilibrium constant for the reaction A(g) ⇌ B(g) is 102 . A reaction mixture...

A.) The equilibrium constant for the reaction A(g) ⇌ B(g) is 102 . A reaction mixture initially contains [A] = 18.6 M and [B] = 0.0 M. Which statement is true at equilibrium? The reaction mixture contains [A] = 18.4 M and [B] = 0.2 M. The reaction mixture contains [A] = 0.2 M and [B] = 18.4 M. The reaction mixture contains [A] = 1.0 M and [B] = 17.6 M. The reaction mixture contains [A] = 9.30 M...

Consider the equilibrium Na2O(s) + SO2(g) ⇌ Na2SO3(s). (a) Write the equilibrium-constant expression for this reaction in terms of partial pressures.

Consider the equilibrium Na2O(s) + SO2(g) ⇌ Na2SO3(s).(a) Write the equilibrium-constant expression for this reaction in terms of partial pressures.(b) All the compounds in this reaction are soluble in water. Rewrite the equilibrium-constant expression in terms of molarities for the aqueous reaction.

Consider the following reaction with an equilibrium constant of 5.10 at 527oC. CO(g) + H2O(g) ⇌...

Consider the following reaction with an equilibrium constant of 5.10 at 527oC. CO(g) + H2O(g) ⇌ H2(g) + CO2(g) If [CO] = 0.150 M, [H2O] = 0.250 M, [H2] = 0.420 M, and [CO2] = 0.370 M, calculate Q. ? Consider the following reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g) Which of the following would not result in a shift towards an increase in production of SO3?pick the correct answer? a)Increase in volume b)Decrease in volume c)Increase in the amount of...

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