2. Convert K, based on concentration, to Kp, based on partial pressures. The term Δn means...
N2(g) + 3 H2(g) ⇌ 2 NH3(g) KP = 6.78 x 105 at 298 K (determined using atm) A 7.5 x 101 L container being held at 298 K is charged with the three gases present in the above equation. Once finished, the initial partial pressure of N2 was 0.59 atm, the initial partial pressure of H2 was 0.45 atm, and the initial partial pressure of NH3 was 0.11 atm. The gas mixture was then allowed to reach equilibrium. Use...
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol), T is the absolute temperature, and Δn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2. A) For the reaction 3A(g)+3B(g)⇌C(g) Kc =...
The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol), T is the absolute temperature, and Δn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2. For the reaction 2A(g)+2B(g)⇌C(g) Kc = 80.2...
1. The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol), T is the absolute temperature, and Δn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2. Part A For the reaction 3A(g)+2B(g)⇌C(g)...
5. The equilibrium constant, KcKc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, KpKp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol)R=0.08206 L⋅atm/(K⋅mol), TT is the absolute temperature, and ΔnΔn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2 For the reaction 3A(g)+2B(g)⇌C(g) KcKc...
Chapter 15 Homework Pressure-Based versus Concentration-Based Equilibrium Constants 11 of 41 Review I Constants I Periodic Table The equilibrium constant, K is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Part A For the reaction 3A(g)3B(g)C(g) Kp = Kc(RT)^n Ke 68.8 ta temperature of 273 C where R 0.08206 L atm/(K.mol), T is the absolute temperature, and...
The equilibrium constant, KcKc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, KpKp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)ΔnKp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol)R=0.08206 L⋅atm/(K⋅mol), TT is the absolute temperature, and ΔnΔn is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g)N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2Δn=2−(1+3)=−2. A For the reaction 3A(g)+3B(g)⇌C(g)3A(g)+3B(g)⇌C(g) KcKc...
The equilibrium constant, KcKcK_c, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, KpKpK_p, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)ΔnKp=Kc(RT)Δn where R=0.08206 L⋅atm/(K⋅mol)R=0.08206 L⋅atm/(K⋅mol), TTT is the absolute temperature, and ΔnΔnDelta n is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)⇌2NH3(g)N2(g)+3H2(g)⇌2NH3(g) for which Δn=2−(1+3)=−2Δn=2−(1+3)=−2. A.) For the reaction 3A(g)+3B(g)⇌C(g)3A(g)+3B(g)⇌C(g)...
A sample of ammonia (NH3) gas is completely decomposed to nitrogen and hydrogen gases over heated iron wool. If the total pressure is 751 mmHg after the reaction, calculate the partial pressures of N2 and H2. Enter your answers in scientific notation. PN2 × 10 mmHg PH2 × 10 mmHg
2. The pressure dependence of the following system at equilibrium was studied at 500°C by measuring the mole fractions of ammonia that were produced at various pressures from 1:3 mixtures of N2 and H2 gases. Assume ideal gas behavior. (Hint: You may assume that the mixtures were prepared from 1 mole of N2 mixed with 3 moles of H2). (10 pts) Ng(g)+H,(g)P NH,(g) P/(bar) 100 XNH3 0.10 200 0.18 300 0.25 400 0.32 500 0.37 600 0.42 700 0.46 800...