Consider the following thermochemical equation: B2H6 (g) + 3 O2 (g) ® B2O3 (s) + 3 H2O (g) DHcomb = – 2035 kJ/mol

Calculate the amount of heat released when 10.0 g of diborane (B2H6) is burned.

Determine the empirical formula of a compound containing 40.6 grams of carbon, 5.1 grams of hydrogen, and 54.2 grams of oxygen. in an experiment, the molar mass of the compound was determined to be 118.084 g/mol. what is the molecular formula of the compound? for both questions, show your work or explain how you determined the formulas by giving specific values used in calculations.

Select the correct answer. given: 2libr + ba → babr2 + 2li in this chemical reaction, 325 grams of barium (ba) react completely. how many moles of lithium (li) are produced? a. 1.18 mol b. 2.37 mol c. 4.73 mol d. 16.4 mol e. 32.9 mol

Asolution contains 180 g of glucose (c6h12o6) and 162 g of water. what is the mole fraction of glucose?