POTENTIALLY MULTIPLE CORRECT ANSWERS FOR EACH
Which of the following is correct?
(a) Exothermic reactions are spontaneous
(b) Reactions with ∆S > 0 are spontaneous
(c) For reactions with increasing number of moles, ∆S > 0
(d) When ∆H > 0, ∆S > 0, with increasing temperature, ∆G will
decrease
Which reaction of the following measured at the standard condition gives ∆G◦f (CO2(g))?
(a) CO(g) + C(s) → CO2 (g)
(b) CO(g)+1/2O2(g)→CO2(g)2
(c) C(s)+O2(g)→CO2(g)
(d) 2C(s)+2O2(g)→2CO2(g)
When a reaction reaches equilibrium, which of the following is correct?
(a) ∆G=0
(b) ∆G◦ = 0
(c) ∆G◦ < 0
(d) ∆G◦ = ∆G
(e) Q=K
(f) lnK=0
At a constant temperature, initially 1.00 mol SO3 was filled into a 1.00 L container , after reaction 2SO2(g)+O2(g) → 2SO3(g) reached equilibrium, number of moles for SO2is 0.60 mol. What is the equilibrium constant K for the above-mentioned reaction?
(a) 2.8
(b) 2.2
(c) 1.5
(d) 1.9
For reaction Cl2(g) + 3F2(g) → 2ClF3(g), what is the relation between the equilibrium constant defined with concentration Kc and the equilibrium constant defined with partial pressure Kp?
(a) Kp = Kc
(b) Kp=Kc(RT)^−1
(c) Kp=Kc(RT)^2
(d) Kp=Kc(RT)^−2
[6] At the same temperature and pressure, consider reactions (1) A + B → 2C, and (2)1 A + 1 B → C, what is the relationship between their standard free energy changes and equilibrium constants
(a) ∆G1 = 2∆G2, K1 = K2
(b) ∆G1 = 2∆G2, K1 = (K2)^2
(c) ∆G1 = ∆G2, K1 = (K2)^2
(d) ∆G1 =∆G2, K1 =K2
Which of the following is true about light?
(a) Light is a wave and a particle at the same time
(b) Photon is quantized electromagnetic radiation
(c) Any object can emit electromagnetic radiation even if it is a blackbody
(d) In photoelectric effect, emitted photoelectron’s kinetic energy is proportional to the. incident photon’s frequency
De Broglie equation of wavelength of matter λ = h/(mv) can be applied to which of the following cases?
(a) When the matter is macroscopic and mass is larger than 1 kg, such as a human
(b) When the matter is microscopic particle and the mass is smaller than an atom
(c) When the matter behaves like a particle
(d) When the matter is traveling in the speed of light
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POTENTIALLY MULTIPLE CORRECT ANSWERS FOR EACH Which of the following is correct? (a) Exothermic reactions are spontaneou...
COULD BE MULTIPLE CORRECT ANSWERS PLEASE HELP MULTIPLE CHOICE (d) 1.9 151 For reaction Cl2(g) + 3F2(g) → 2CIF3(g), what is the relation between the equilibrium constant defined with concentration Kc and the equilibrium constant defined with partial pressure Kp? (a) K = K (b) K = K (RT) -1 (c) Kp = K (RT)2 (d) Kp = Kc(RT)-2 [6] At the same temperature and pressure, consider reactions (1) A+B 2C, and (2) A+ B+C, what is the relationship between...
POTENTIALLY MULTIPLE CORRECT ANSWERS ( 1 ) [6] At the same temperature and pressure, consider reactions (1) A+B → 2C, and (2) A+B+C, what is the relationship between their standard free energy changes and equilibrium constants? (a) AG] =2AG2, ki = K2 (b) AG1 = 2AG2, K1 = (K2)2 (c) AG = AG2, K1 = (K2) (d) AG = AG2, k = K2 [7] Which of the following is true about light? (a) Light is a wave and a particle...
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related to the following reaction? O2 (a) N2(a) + O2(a) = 2NO(a) K=.............. (b) 4NOQ = 2Nz () + 2O2(g) Kos......... (c) NO) 1/2 N2(0)+ 1/2O2(0) K3= +++ (d) 1/2 N2(a) + 1/2O2(a) = NO) Ke=.............. 3. Given Kc or ko for the following reactions, what is the value of Koor K? (a) l2(g) + Cl2(a) = 2ICIOX Kc = 2.0 x105 at 25°C (b)...
Part A Determine the value of the equilibrium constant, Kgoal, for the reaction CO2(g)⇌C(s)+O2(g), Kgoal=? by making use of the following information: 1. 2CO2(g)+2H2O(l)⇌CH3COOH(l)+2O2(g), K1 = 5.40×10−16 2. 2H2(g)+O2(g)⇌2H2O(l), K2 = 1.06×1010 3. CH3COOH(l)⇌2C(s)+2H2(g)+O2(g), K3 = 2.68×10−9 Express your answer numerically. Part B Determine the equilibrium constant, Kgoal, for the reaction 4PCl5(g)⇌P4(s)+10Cl2(g), Kgoal=? by making use of the following information: P4(s)+6Cl2(g)⇌4PCl3(g), K1=2.00×1019 PCl5(g)⇌PCl3(g)+Cl2(g), K2=1.13×10−2 Express your answer numerically.
Given that K1 and K2 are the respective equilibrium constants for the two reactions CO2(g) + H2(g) = CO(g) + H2O(l) K1 = 3.08×10-4 CdO(s) + H2(g) = Cd(s) + H2O(l) K2 = 40.7 Determine the equilibrium constant for the reaction CO(g) + CdO(s) = CO2(g) + Cd(s) K =
Determine the value of the equilibrium constant,Kgoal , for the reaction CO2(g)--->/<--- C(s)+O2(g), Kgoal=? by making use of the following information: 1. 2CO2(g)+2H2O(l)--->/<--- CH3COOH(l)+2O2(g), K1=5.40x10^-16 2. 2H2(g)+O2(g)--->/<--- 2H2O(l), K2=1.06x10^10 3. CH3COOH(l)--->/<--- 2C(s)+2H2(g)+O2(g), K3= 2.68x10^-9 Kgoal=_______
Question 2 of 3 Two reactions and their equilibrium constants are given. A+2B 2C K1 2.77 2C D K2 0.198 Calculate the value of the equilibrium constant for the reaction D A + 2 B. K =
Part A Determine the value of the equilibrium constant, Kgoal, for the reaction C(s)+1/2O2(g)+H2(g)<-->1/2CH3OH(g)+1/2CO(g), Kgoal=? by making use of the following information: 1. CO2(g)+3H2(g)<-->CH3OH(g)+H2O(g) K1 = 1.40 x 10^2 2. CO(g)+H2O(g)<-->CO2(g)+H2(g) K2 = 1.00 x10^5 3. 2C(s)+O2(g)<-->2CO(g) K3 = 2.10 x10^47 Express your answer numerically Kgoal = ? Part B Determine the equilibrium constant, Kgoal, for the reaction 4PCl5(g)<-->P4(s)+10Cl2(g), Kgoal =? by making use of the following information: 1. P4(s)+6Cl2(g)<-->4PCl3(g) K1 = 2.00 x10^19 2. PCl5(g)<-->PCl3(g)+Cl2(g) K2 = 1.13x10^-2 Express...
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)?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...