Which of the following conceptually assesses the extent to which a brand has delivered value in exchange for the attachment fans have awarded it?

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Answer the following question.  120.0g  of helium occupies a 15.25 L cylinder which is heated until the pressure is 150 atm. What is the temperature (in oC) of the gas? Chose your final answer here. After submitting the exam, upload the matching calculations to the Exam 4 Solutions, Extra Credit, and Partial Credit assignment. Answer – 2pts, work – 2pts

In the Crash Course video (War and National Building in Latin America), John Green discusses reasons why Latin American nation state have had difficulty creating stability and national cohesion.  Describe TWO of these reasons in as much detail as possible (covering more of issues he discusses can result in a higher-than-perfect score).

Use Hess’s law to calculate the enthalpy of reaction for the target reaction (Hint: Do not forget about the coefficients)    2 F2(g) + 2 H2O(l) => 4 HF(g) + O2(g) from: H2(g) + F2(g) => 2 HF(g);                      ΔHo  = -542 kJ2 H2(g) + O2(g) => 2 H2O(l);                 ΔHo  = -572 kJ Submit the answers in this exam. After submitting your exam, take the pictures of your work and upload them to Exam 4 Solutions, Extra Credit, and Partial Credit assignment. Your work must reflect the answer provided here. NO CREDIT will be awarded for the answer without work or justification shown. Answer:

Consider the balanced equation and answer the questions below.  2C2H2 (g)  + 3O2 (g) =>4CO (g) +2H2O (l)   How many moles of water will form if 8.0 moles of O2 is used? (4)  If 15.0 moles of C2H2 is used, how many grams of water will form?(4) How many molecules are in 4.50 grams of C2H2? (1) What is the molarity of a solution prepared by dissolving 1.50g of C2H2 in 825mL of the non-aqueous solution? (4) How many moles of oxygen are needed to burn 1.2044 x1024 molecules of C2H2?(1)  Which reagent is a limiting reagent (1) and how many moles of CO form when 15.0 mol C2H2 react with 25.0 mol of O2?(4)  Which reagent is a limiting reagent (2) and what is the theoretical yield in grams o CO (3) when 25.0 g C2H2 react with 25.0 g of O2? If  25.5 g of CO formed in reaction, what are the  actual(1), and percent(1) yields of CO? Submit the answers in this exam. After submitting your exam, take the pictures of your work and upload them to Exam 3 Solutions, Extra Credit, and Partial Credit assignment. Your work must reflect the answer provided here. NO CREDIT will be awarded for the answer without work or justification shown. Answers:

Answer the following question.   Consider a buffer solution that is 0.600M formic acid(HCOOH) and 0.350M sodium formiate. Ka (formic acid) = 1.87 x10-4(10 pts) Calculate the [H+], [OH-], pH, and pOH for this buffer. (10pts) Calculate the pH of this buffer after adding 22.0 mL of 2.2M NaOH to 1.0 L of the solution (Hint: 1.0 L + 22 mL = 1.0 L according to the rules of addition for s.f.).(2pts) Submit your final answers here. After submitting the exam, upload the matching calculations to the Exam 3 Solutions, Extra Credit, and Partial Credit assignment.  

Use the properties of enthalpy as a state function (version of Hess’s law) and  data below to calculate the enthalpy change for the given reaction (Hint: Do not forget about the coefficients)    Standard Enthalpies of Formation, in kJ/mol ΔHof     ΔHof NO(g)       +90.25          NO2(g)      +33.2        NH3(g)     -45.9     N2O(g)        81.6   H2O(l)        -285.8         H2O(g)         -241.8 Use the properties of enthalpy as a state function (version of Hess’s law) and  data above to calculate the enthalpy change for the reaction (Hint: Do not forget about the coefficients):                                          6 NO2(g)  +  8 NH3(g)  =>  7 N2(g)  +  12 H2O(g)                      ΔH = ? Submit the answers in this exam. After submitting your exam, take the pictures of your work and upload them to Exam 4 Solutions, Extra Credit, and Partial Credit assignment. Your work must reflect the answer provided here. NO CREDIT will be awarded for the answer without work or justification shown. Answer:

Answer the following question.  15.3 g of KClO3 decomposes according to the following balanced equation. Use the stoichiometry and gas laws to determine the volume of O2 formed at 1 atm and 500K. The molar mass for KClO3 is 122.55 g/mol.                 2 KClO3(s)  →  2 KCl(s) + 3 O2(g) Submit the answers in this exam. After submitting your exam, take the pictures of your work and upload them to Exam 4 Solutions, Extra Credit, and Partial Credit assignment. Your work must reflect the answer provided here. NO CREDIT will be awarded for the answer without work or justification shown. Answer:  

Consider the balanced equation and answer the questions below.  2C2H6 (g)  + 5O2 (g) =>4CO (g) + 6H2O (l)     How many moles of water will form if 12.0 moles of O2 is used? (4)  If 5.0 moles of C2H6 is used, how many grams of water will form?(4) How many molecules are in 5.50 grams of C2H6? (1) What is the molarity of a solution prepared by dissolving 2.50g of C2H6 in 725mL of the non-aqueous solution? (4) How many moles of oxygen are needed to burn 1.1011 x1024 molecules of C2H6?(1)  Which reagent is a limiting reagent (1) and how many moles of CO form when 12.0 mol C2H6 react with 32.0 mol of O2?(4)  Which reagent is a limiting reagent (2) and what is the theoretical yield in grams of CO (3) when 20.0 g C2H6 react with 20.0 g of O2? If  12.5 g of CO formed in reaction, what are the  actual(1), and percent(1) yields of CO? Submit the answers in this exam. After submitting your exam, take the pictures of your work and upload them to Exam 3 Solutions, Extra Credit, and Partial Credit assignment. Your work must reflect the answer provided here. NO CREDIT will be awarded for the answer without work or justification shown. Answers: