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. 18.3 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)

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. 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):                                         8 NO2(g)  + 6 NH3(g)  =>  7 N2O(g)  +  9 H2O(g)                      ΔH = ?  

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 Fe(s) + 3 Cl2(g) => 2 FeCl3(s)        from Fe(s) + Cl2(g) => FeCl2(s);                ΔHo  = -341.8 kJ2 FeCl3(s) => 2 FeCl2(s) + Cl2(g);     ΔHo  = +115.4 kJ  

At constant pressure, the sign of q for the process CO2(g) => CO2(s) is____, because______

If you remove some ice from an of an ice-water mixture,

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 Fe(s) + 3 Cl2(g) => 2 FeCl3(s)        from Fe(s) + Cl2(g) => FeCl2(s);                ΔHo  = -341.8 kJ2 FeCl3(s) => 2 FeCl2(s) + Cl2(g);     ΔHo  = +115.4 kJ  

The following is an explanation of the higher boiling of NH3 compared to PH3

What volume of methane in L, CH4, has the same number of moles of gas as 10  L of CO2 gas at the same temperature and pressure?

The following can be used to measure the heat of combustion for an unknown sample?

The following phase change is exothermic: