Determine the formula mass for Gold (IV) oxide an imaginary compound. (Enter your answer with 4  sig figs and no units).  

What type of reaction is the following? Ca(OH)2(s) + 2 HNO3(aq) 

The mass of a graduated cylinder is [m] grams.  After adding an unknown liquid to it, total mass became [n] grams.  The volume of the liquid is shown below (in mL).  What’s the density of the unknown liquid? (enter your answer with 3 decimal places and no units, the understood unit is g/mL)      

The volume occupied by 1.5 mol of gas at 35°C and 2.0 atm pressure is __________ L.

Classify the reaction below. FeCl3(aq)  +  3 NaOH(aq) 

Sodium hydride reacts with excess water to produce aqueous sodium hydroxide and hydrogen gas. How many grams of NaH will produce 0.923 L of gas at 23.5oC and a barometric pressure of 765 torr, when the hydrogen is collected over water. The vapor pressure of water at this temperature is 28 torr.  NaH (s) + H2O (l) → NaOH (aq) + H2 (g)

Zinc reacts with aqueous sulfuric acid to form hydrogen gas according to the reaction below.  In an experiment, 0.225 L of wet H2 is collected over water at 26.9oC and a barometric pressure of 748 torr. How many grams of Zn have been consumed? The vapor pressure of water at this temperature is 26.74 torr. Zn (s) + H2SO4 (aq) → ZnSO4 (aq) + H2 (g)

How many milliliters of 0.152 M Ba(OH)2 are required to neutralize 20.00 mL of 0.263 M HCl, according to the reaction below? Ba(OH)2 (aq) + 2 HCl (aq) → BaCl2 (aq) + 2 H2O (l)

Calculate the ΔH°rxn of combustion of C3H6(g),                   C3H6(g)  +  9/2 O2(g) 

In an experiment, a student placed a beaker on a balance and the mass of the beaker was 132.5 grams.  The student then added some copper to the beaker, the mass increased to 147.3 grams.  How many moles of copper did the student have? (enter your answer with 3 decimal places and no units, the understood unit is mole)