w2019-practice

Activated complex 400 (b) 300 Products Potential Energy (a) 200 (c) 100 Reactants Reaction Pathway Activated complex 400 (b) 300 Products Potential Energy (a) 200 (c) 100 Reactants Reaction Pathway Alex thinks that the graph above represents an exothermic reaction and the AH = +400kJ and energy will be released in this reaction. Is Alex correct? If not, find his error and then correct it with explanation. %3D

Construct the expression for Kc for the following reaction. Drag the tiles into the numerator or denominator to form the expression. Each reaction participant must be represented by one tile. Do not combine terms. PLOY JOHY 24.01 H.O (1) H (aq) + OH (aq) K₂ = HOP P+1 201 pry JOH RESET 201

Name: Date: Section: Prelaboratory Assignment: Spectrophotometric Determination of an Equilibrium Constant. 1. At 227°C, carbon monoxide gas reacts with hydrogen gas to form one mole of methanol, CH,OH. At equilibrium, the partial pressures of the gases are Pco= 0.295 atm, PH2 1.25 atm, and PCH3OH = 2.18 atm. a) Write a balanced equation for the reaction b) Calculate the equilibrium constant for the reaction. 2. Consider the reaction: A+B=C+ 3D A solution was prepared by mixing 50.00 mL of 1.00 x 10³ M A, 100 mL of 2.00 x 10 MB, 10.0 mL of 1.0 M C and 75 mL of 1.50 x 10³M D. At equilibrium, the concentration of D was measured to be 6.0 x 10 M. a) Calculate the equilibrium concentrations of each species b) Calculate the equilibrium constant. 3. Consider the reaction: # 2NO2(g) + Cl2(g) 2NOCI The initial pressure of NO, was 1.577 atm and the initial pressure of Cl₂ was 0.427 atm. At equilibrium, the partial pressure of NOCI is 0.624 atm. Calculate K.

he 10.2. Suppose that a reaction A + 2B = 2Y + 2Z is believed to occur according to the mechanism k₁ A 2X (very rapid equilibrium) k₂ X+BY+Z (slow) Obtain an expression for the rate of formation of the product Y.

For the reaction N2(9) + O2(9) = 2NO(g) classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the reaction. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help halve Po2 halve double PN2 double halve PN2 double Po2 PNO PNO Leftward shift Rightward shift No shift

The equilibium constants of the reactions  FeO(s)  + CO(g)  = Fe(s) + CO2(g)   ; K1 FeO (s) + H2(g)  = Fe(s) + H2O (g) ; K2 Temp (oC)   600      700     800      900     1000 ------------------------------------------- K1               0.900  0.673   0.535   0.453   0.396 K2               0.332   0.422  0.499   0.594   0.668 Calculate the Equilibium constant of the reaction CO (g) + H2O (g)  = CO2(g) + H2(g)   at the above temperature   Also calculate the heat of the reaction for the production of hydrogen from carbon monoxide and water vapour, assuming it to be independent of temperature

PLAY General Chemistry I Laboratory Manual, 2019 Revision 119 2) Calculate AH for the reaction below using Hess' law. and the C2H6(g) → C2H2(g) + H2(g) Introde AH=? Youhe C2H2(g) +5/202(g) → 2CO2(g) + H2O(1) AH = -1300 kJ 2H2(g) + O2(g) → 2H2O(1) ΔΗ--572 kJ 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(1) AH = -3120 kJ ithin atom -16022 10 Wen

Consider the acid catalyzed reaction; AH + H+ ----> AH,+ rate = k1[AH][H*] (fast) AH2+ ----> AH + H+ rate = k2[АН2*] (fast) AH,+ + B ----> BH+ + AH rate = k3[AH2*[B] (slow) Using the pre-equilibrium approximation derive the rate law. rate = (kık3/k2)[H*][B] rate = (kık2/k3)[HA][H*[B] rate = (kık3/k2)[HA][H+][B] rate = (kık3/k2)[HA][B] If the only source of H+ is from HA show that it is possible to derive a rate law that is independent of H+. What is the rate law? Hint: Add the fast equilibrium HA H+ + A¯ to the proposed mechanism in part a). (kık3Ka/2/k2)[HA]!/2[B] (kık3Ka1/2/k2)[HA]3/2[B] rate = (kık3/k2K1/2)[HA][B] rate = (kık3/k2Ka1/2)[HA]3/2[B] rate = rate =

C. BaCl2(aq)+ K2CrO4(aq)<---> BaCrO4(s)+ 2K+(aq)+ 2Cl-(aq) and 2CrO42-(aq)+ 2H+(aq)<---> Cr2O72-(aq)+ H2O(l) For the questions indicate where reaction will shift towards reactant or  product and tell the color observed. 1. Place approximately 5 mL of 0.1 M BaCl2(barium chloride) solution in a test tube.(Note color) Add several drops of 1 M K2CrO4and note the result. 2. Add 6 M HCl until you observe a significant change in the above solutio

ID=182385216 Kinetics For Practice 14.4 - Enhanced - with Feedback I Review | Constants Cyclopropane rearranges to form propene in the gas phase. v Part A If the initial cyclopropane concetration is 0.0415 M, what is the cyclopropane concentration after 280 minutes? Express your answer with the appropriate units. CH2 CH3-CH=CH, Value Units H2C-CH2 The reaction is first order in cyclopropane and has a at 720 K. Submit Request Answer measured rate constant of 3.36 x 10-5 You may want to reference (Pages 598 - 605) Section 14.5 while completing this problem. Dreuid.

Potential energy (k) Potential energy (kJ) cument identifier=D7b0cf258-fde2-45f0-ba86-cffe2fe86028&filename%38.03%20Collision%20Theory%20and%20Read New Tab Spotify- Liked Songs Application: Chemical Kinetics 1) The graph below is a potential energy diagram for the hypothetical reaction: 2) On the graph below, draw a potential energy diagram for the following reaction: A + B C + D Q + R S + T given the following information: PE of Q+ R= 150 kJ PE of S+ T = 250 kJ PE of the activated complex = 375 kJ 06 09 40. 30, 2 350 Reaction coordinate 000 Is the forward reaction endothermic or exothermic? Calculate the value of AH for this reaction. Reaction coordinate b. What is the value of the potential energy of the activated complex? a. Is the forward reaction endothermic or exothermic? Calculate the value of AH for this reaction. c. Calculate the activation energy (EA) for the forward reaction. b. Calculate the EA for the forward reaction.. d. Draw a dashed line to show the effect of adding a…

Differential EQN: Bruce Wayne analyzes a kryptonite in order to prepare if ever Clark Kent becomes rogue. The former studieda kryptonite and found that it decomposes at a rate proportional to the quantity of kryptonite present.Suppose that it is found that in 25 years approximately 1.1% of a certain quantity of kryptonite hasdecomposed. Determine how long it will take until 50% of the original amount of kryptonite dissipates. pls. provide complete solution with explenation. the formula we use is : dx/dt=kx

The progress of a reaction is determined by various steps involving energy changes with respect to collision theory. Identify the key features of the reaction profile below. Drag the appropriate labels to their respective targets in the energy profile diagram.

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1) Use Hess's Law to determine AH for the following target reaction. 3 CO₂(g) + 4 H₂O(g) b) C3Hg(g) + 5 O₂(g) C(s) + O₂(g) -CO₂(g) 2 H₂(g) + O₂(g) 3 C(s) + 4 H₂(g) →→→ 2 H₂O(g) C3H8(g) AH = AH = ΔΗ ΔΗ = ??? -2043 kJ -393.5 kJ -483.6 kJ

Apple Google Disney ESPN Yahoo! ☆ Consider the reaction: Substance Ca(OH)2 (aq) HCl(aq) CaCl₂ (s) H₂O(1) ASO = system Submit Answer Biomedical Careers Program J/K B prod03-cnow-owl.cengagenow.com Sº (J/K mol) -74.5 56.5 104.6 69.9 Retry Entire Group Apple iCloud Yahoo Images Bing Google Wikipedia b ☆ G [Review Topics] D2L D2L 4 more group attempts remaining D2L [References] Use the References to access important values if needed for this question. Facebook Twitter LinkedIn Ca(OH) 2 (aq) + 2HCl(aq) → CaCl₂ (s) + 2H₂O(1) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.73 moles of Ca(OH)2 (aq) react at standard conditions. COWLv2... D2L b The Weather Channel Yelp TripAdvisor C D2L M G + 88 M ?

Where: [A]o 1 [A] = = [A] = of reactant A initial kt+ concentration 1 [A]o concentration of reactant A 1 [AO] k = rate constant t = time In order to solve for the time, t, in two steps you must: Step One Add the same expression to each side of the equation to leave the term that includes the variable by itself on the right-hand side of the expression: (Be sure that the answer field changes from light yellow to dark yellow before releasing your answer.) 1 [A]o Drag and drop your selection from the following list to complete the answer: + 1 [A] = [Ao] 1 [Ao] +kt+ -[Ao] Previous Next

Draw a dashed line to show the effect of adding a catalyst to the system

A reaction at 21.0 °C evolves 552. mmol of dinitrogen difluoride gas. Calculate the volume of dinitrogen difluoride gas that is collected. You can assume the pressure in the room is exactly 1 atm. Round your answer to 3 significant digits. volume: L x10 Submit Assignmer Continue 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center I Accessibility IMG-4472.jpg IMG-4471.jpg IMG-4467.jpg IMG-4464.jpg IMG-4474.jpg MacBook Air DII DD 80 F7 F8 F9 F10 F11 F1 F2 F3 F4 F5 F6 # $ % & ) 1 2 3 4 5 6 7 8 9

Construct the expression for Kc for the following reaction. 2 Sb(s) + 5 CL(g) =2 SbCls(g) Drag the tiles into the numerator or denominator to form the expression. O RESET 2[SDCL] 2[SbClj? [CL] 5[CL] [Sb] 2[Sb] [SbF 2[Sb] 46°F a earch 近

Consider the following elementary reaction: N2O(g) -> N2(g) + O(g) Suppose we let k1 stand for the rate constant of this reaction, and k-1 stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of N2O in terms of k1, k-1, and the equilibrium concentrations of N2 and O

I was instructed to balence the equation of HCl(aq) + NaHCO3(aq) which yields to H20(l) + CO2(g) +NaCl(aq).  However, I am pretty sure this equation is already balenced, but I am confused.