22)
Δ n = number of gaseous molecule in product - number of gaseous molecule in reactant
use:
Kp= Kc (RT)^Δn
For Kp = Kc,Δn should be 0
Answer: E
Only 1 question at a time please
Q(22) Kp=Kc when? A) The reaction is at equilibrium B) The reaction is exothermic C) The reaction is endothermic D)...
Q(18) NI(CO)49) - Ni(s) + 4 CO(g)Adding nickel (solid) to this reaction will cause the equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it depends on the amount added Q(19) CO2 + H2 -CO + H2O Adding a catalyst to this reaction will cause the COD at equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it...
Q(17) Which species is amphiprotic? A) H3PO4 C) PO43- D) None of these B) H2PO4 Q(18) Ni(CO)4(g)Nis)+ 4 CO(g)Adding nickel (solid) to this reaction will cause the equilibrium to C) remain unchanged E) it depends on the amount added B) Shift toward the reactants A) Shift toward the products D) increase the temperature Q(19) CO2 H2 CO + H20 Adding a catalyst to this reaction will cause the [CO] at equilibrium to A) Shift toward the products C) remain unchanged...
A) No change in the equilibrium C) More information is needed to answer the question. B) Equilibrium shifts to the right. D) Equilibrium shifts to the left E) None of the answers is correct. Q(17) Which species is amphiprotic? A) H3PO B) H2PO D) None of these C) PO Q(18) Ni(CO)4)Nie)+ 4 COlaAdding nickel (solid) to this reaction will cause the equilibrium to A) Shift toward the products C) remain unchanged E) it depends on the amount added B) Shift...
A Q=K: the reaction mixture is at equilibrium O T OM B. Q<K; the reaction will shift towards the reactants C. Q>K; the reaction will shift towards the products → KA А е е D. Q>K; the reaction will shift towards the reactants MOL (E. Q<K; the reaction will shift towards the products. M280. 00 3. For the reaction M SES00.0 3 to noiriwa H2 (9)+CO2(9) <==> H20 (9) +CO (9) Kc = 0.798 at 320°C. 0.492 moles of H2...
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...
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)?n where R=0.08206 L?atm/(K?mol), T is the absolute temperature, and ?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) for which ?n=2?(1+3)=?2. Part A For the reaction 3A(g)+3B(g)?C(g) Kc...
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)...
) Given the following reaction at equilibrium, if Kp = 1.10 at 250.0 °C, Kc = ________. PCl5 (g) PCl3 (g) + Cl2 (g) A) 1.10 B) 2.56 × 10 -2 C) 47.2 D) 42.9 E) 3.90 × 10 -6
. 5. A reaction with an equilibrium constant Kc = 1.5 x 10-25 would consist of which of the following at equilibrium:sep . A) some reactants and products with reactants slightly favored B) essentially all reactantsisèp(0.5 pt) C) approximately equal reactants and products to D) some reactants and products with products slightly favored E) essentially all productssep . F) exactly equal amounts if reactants and products