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Enter your answer in the provided box. For the reaction N2(g) + 3H2(g)⇆ 2NH3(g) KP is 0.000205 at 563°C. What is Kc for the reaction? Kc =
Enter your answer in the provided box. For the reaction N2(g) +3H2(g)* 2NH3(g) Kp is 0.000667 at 327°C. Wha is Kc for the reaction?
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)...
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)...
2. At 55°C, the equilibrium constant for the reaction N2(g) + 3H2(g) + 2NH3(g) is Kp=0.05. What is the equilibrium constants Kc and Kp for the reaction 4NH3 + 2N2(g) + 6H2(g)? Kp = 400 Kc = 7.62 x 10 3. For the reaction given below, 10.00 moles of A and 25.00 moles of B are placed in a 5.00-L container at 120 °C. A(g) +2B(g) → C(g) At equilibrium, the concentration of A is 0.5 mol/L. What is the...
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 =...
23 A) For the reaction 2CH4(g)⇌C2H2(g)+3H2(g) Kc = 0.130 at 1651
∘C . What is Kp for the reaction at this temperature?
23 B) For the reaction N2(g)+3H2(g)⇌2NH3(g) Kp= 3.40×10−3 at 292
∘C. What is Kc for the reaction at this temperature?
Part A For the reaction 2CH (g) = C2H2(g) + 3H2(g) Kc = 0.130 at 1651 °C. What is K, for the reaction at this temperature? Express your answer numerically. View Available Hint(s) V AC ? K Kp...
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...