Directions: Use the label provided to answer the following questions. Order: Albuterol 1.2 mg p.o. t.i.d. is ordered for a child weighing 27 lb. The recommended dosage is 0.3 mg/kg/24 hr divided in q8h doses.   How many milliliters of albuterol are needed to administer the first TID ordered dosage? _____ mL

Answer the following question. Show the answer on the screen provided. After uploading your exam, take the picture of your work and upload it 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 shown. 12.3 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)

On the generic phase diagram below, the liquid is present at the temperatures and pressures which are the coordinates of the following points:

Considering the limiting reactant, how much heat is produced at constant pressure if 0.243 g of magnesium reacts with 100.0 mL of 0.300 M HCl according to the reaction below? Mg(s) + 2HCl(aq) => MgCl2(aq) + H2(g); ΔHo = –462.5 kJ

Calculate the ΔH  for the following reaction using the given bond energies. Show work for credit (H – F = 565 kJ; O – O = 494 kJ; H – O = 463, O – F = 184). F2O(g) + H2O(g) => O2(g) + 2 HF(g)

The following combination of signs for heat and work (respectively, heat first, work, next in the answer) represents a system that is gaining heat from the surroundings, and surroundings are doing work on the system?      

Answer the following question. Show the answer on the screen provided. After uploading your exam, take the picture of your work and upload it 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 shown. Use Hess’s law to calculate the enthalpy of reaction for the target reaction N2(g) + O2(g) => 2 NO(g) 4 NH3(g) + 5 O2(g) => 6 H2O(l) + 4 NO(g);     ΔHo/kJ = -6134 NH3(g) + 3 O2(g) => 2 N2(g) + 6 H2O(l);      ΔHo/kJ = -790  

Use  bond enthalpies (in kJ/mol):  C-C    348    C=C    614    C≡C   839          H-H  436              C-H   413          O-H  463                     C-O 358                  C=O    799                      to estimate ΔH for the reaction      H2C=CH–CH2–OH (g)  =  >  HC≡C–CH=O(g)  + 2 H2(g)           SHOW WORK FOR CREDIT 

Answer the following question. Show the answer on the screen provided. After uploading your exam, take the picture of your work and upload it 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 shown. Use Hess’s law to calculate the enthalpy of reaction for the target reaction 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  

Question 4 (10 points) Find the inverse Laplace transform