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)

A chemical reaction that gives off energy in the form of heat is considered _____.

The following intermolecular forces exist between the molecules of NH3 and acetone (CH3)2C=O:

A  75.0 L balloon contains 215.18 g of neon at 27oC. Calculate the pressure in atm,  in the ballon.

A 0.213 g sample of an organic compound with a molar mass of 386.0 g/mol was burned in the bomb calorimeter with a heat capacity of 2.54 kJ/K. The temperature in the calorimeter increased by 4.12 K. Calculate the energy of combustion of the compound in kJ/mol.

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,