Please balance the given reaction. Calculate how many grams of O2(2) are produced from the decomposition of 2 moles of potassium chlorate addressing to the stochiometry? H3PO4 + CaO→ Ca3(PO4)2 +H2O KC103()→ KClo = 02e]
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- A chemist at a pharmaceutical company is measuring equilibriumconstants for reactions in which drug candidatemolecules bind to a protein involved in cancer. The drugmolecules bind the protein in a 1:1 ratio to form a drug–proteincomplex. The protein concentration in aqueous solutionat 25 °C is 1.50 x 10-6 M. Drug A is introduced into the proteinsolution at an initial concentration of 2.00 x 10-6 M.Drug B is introduced into a separate, identical protein solutionat an initial concentration of 2.00x 10-6 M. At equilibrium,the drug A–protein solution has an A–protein complexconcentration of 1.00 x 10-6 M, and the drug B solutionhas a B–protein complex concentration of 1.40 x 10-6 M.Calculate the Kc value for the A–protein binding reactionand for the B–protein binding reaction. Assuming that thedrug that binds more strongly will be more effective, whichdrug is the better choice for further research?For the reaction A + B <=> AB, kassoc = 2.0 sec-1 M-1 and kdissoc = 0.5 sec-1. This means that Kassoc is equal to ____ M-1. (Enter your answer to the nearest 0.1; do not include units)The value of KC for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 × 10-4 at 1400 K.2H2S(g)<--->2H2(g)+S2(g) A sample of gas in which [H2S] = 3.85 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in the original sample.
- The value of KC for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 × 10-4 at 1400 K. 2H2S(g)⇌2H2(g)+S2(g) A sample of gas in which [H2S] = 3.45 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in the original sample.Consider the reaction Mn+ + ne- ⇌ M. If ΔG*c = ΔG* + (1-α)nFE and η = E – Eeq, prove that ic = io exp[-(1-α)nFηa)/RT)].Consider the reaction CO32-(aq) + H2O(l) HCO3-(aq) + OH–(aq). Kb for CO32- is 2.1 × 10–4 at 25°C. What is Ka for the HCO3- ion at 25°C?
- Consider the reaction between bromine and chlorine gases to form bromochloride: Br2(g)+Cl2(g)⇌2BrCl(g), Kc=1.11×10−4Br2(g)+Cl2(g)⇌2BrCl(g), Kc=1.11×10−4 at 150K150K A reaction vessel contains 0.20M Br20.20M Br2, 0.35M0.35M Cl2Cl2, and 3.0×10−3M BrCl3.0×10−3M BrCl. Calculate the reaction quotient, QQ, and determine in which direction the reaction proceeds to reach equilibrium. View Available Hint(s) Consider the reaction between bromine and chlorine gases to form bromochloride: at A reaction vessel contains , , and . Calculate the reaction quotient, , and determine in which direction the reaction proceeds to reach equilibrium. a. 4.3×10–24.3×10–2, the reaction system proceeds to the left b. 1.1×10–41.1×10–4, the reaction system is at equilibrium c. 1.3×10−41.3×10−4, the reaction system proceeds to the left d. 1.3×10–41.3×10–4, the reaction system proceeds to the rightFor a certain reaction, Kc�� = 9.80×10−10 and kf=�f= 2.59×10−5 M−2⋅s−1�−2⋅s−1 . Calculate the value of the reverse rate constant, kr�r, given that the reverse reaction is of the same molecularity as the forward reaction. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋅s−1�−2⋅�−1 include ⋅⋅ (multiplication dot) between each measurement. View Available Hint(s) For a different reaction, Kc�� = 5.40×102, kf=8.96×103s−1�f=8.96×103s−1 , and kr=�r= 16.6 s−1s−1 . Adding a catalyst increases the forward rate constant to 2.05×106 s−1s−1 . What is the new value of the reverse reaction constant, kr�r, after adding catalyst? Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋅s−1�−2⋅�−1 include ⋅⋅ (multiplication dot) between each measurement. View Available Hint(s)Initial temp: 19.06 C 0.5 M concentration 200 mL of HCl and 200 mL of NaOH are combined in an insulated container. H+(aq) + OH-(aq) - - -> H2O (l) ∆H H++ = 0, ∆H OH−− = -230 kJ/mol, ∆H H2O = -286 kJ/mol ∆H reactants = ∆H H++ + ∆H OH−− = -230 + 0 = -230 kJ/mol ∆H reactants = -286 kJ/mol - ( -230 kJ/mol) = -56 kJ/mol H+ (aq) + OH− (aq) - - -> H2O (l) Using your observations and the stoichiometric relationships of the reaction, determine the number of moles that react. Show/upload your work.
- For the decomposition of phosphorous pentachloride to phosphorous trichloride and chlorine at 400K the KC is 1.1x10-2. Given that 1.0g of phosphorous pentachloride is added to a 250mL reaction flask, find the percent decomposition after the system has reached equilibrium. PCl5(g) <---> PCl3(g) + Cl2(g)Some sulfuric acid is spilled on a lab bench. You can neutralizethe acid by sprinkling sodium bicarbonate on it and thenmopping up the resulting solution. The sodium bicarbonatereacts with sulfuric acid according to:2 NaHCO31s2 + H2SO41aq2¡Na2SO41aq2 +2 H2O1l2 + 2 CO21g2Sodium bicarbonate is added until the fizzing due to the formationof CO21g2 stops. If 27 mL of 6.0 M H2SO4 was spilled,what is the minimum mass of NaHCO3 that must be addedto the spill to neutralize the acid?In a lab experiment, a student manages to dissolve 0.00250 moles of a mysterious compound AB into 1 L of water. The mysterious compound dissociates using the following equation: AB(S) ⇌ A(aq) + B(aq) What is the value of the Ksp for this compound? (Please provide your answer to 3 significant figures in scientific notation such as 1.23*10^-5.)