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.

Which one of these compounds is an ionic compound?

What is the net ionic equation for the following molecular equation? BaCl2(aq) + K2SO4(aq) →   BaSO4(s)+ 2KCl(aq)

If the heat produced by the reaction of combustion of 1 mole of ethanol is 8 kJ/mol, (see the thermochemical equation below), how much heat in kJ is produced by the combustion of 155 g of ethanol at the same conditions (MMethanol= 46.07 g/mol)? C2H6O(g) + 3O2(g)  → 2CO2(g) + 3H2O(g);       ∆H°rxn=−1366.8 kJ/mol  

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?

Consider the following balanced reaction: Pb(s) + 2 Cl2(g)  → PbCl4(s) Starting with 30.0g of Cl2 (MMCl2= 70.90 g/mol) and excess Pb, determine the theoretical yield of PbCl4(MMPbCl4= 349.01 g/mol).

What is the percent by mass of oxygen in (NH4)2SO3?

Which is the correct coefficient for O2 in the following equation after balancing?       _C4H10  +  _O2  →  _CO2 + _H2O

Use the Lewis dot structure (make sure you show all electron pairs) to predict the electronic geometry (EG) and the shape of the molecule H2O?

Convert 1.35 atm to mm Hg.