Acid precipitation dripping on limestone produces carbon dioxide by the following reaction:  CaCO3​(s)+2H+(aq)>>>>Ca2+(aq)+CO2​(g)+H2​O(l) 14.5  mL of CO2 was produced at 25.0°C and789.0  mm Hg.   How many moles of CO2 were produced?     How many milligrams of CaCO3 were consumed?

The catalytic decomposition of hydrogen peroxide yields oxygen gas and water, according to the reaction given below. In an experiment, the decomposition of hydrogen peroxide yielded 75.3 mL of gas collected over water at 25°C and 0.976 atm. (Pwater = 0.032 atm at 25°C) 2 H2O2(aq) → 2 H2O(l) + O2(g) If the original H2O2 solution had a volume on 500 mL, what was the molar concentration of hydrogen peroxide prior to decomposition?                          A)    1.8 * 10-4 M                                B)    0.058 M                        C)    0.0062 M                        D)    0.060 M                        E)    0.012 M

Hydrogen gas is produced by the reaction between metallic aluminum and aqueous hydrochloric acid. 2 Al(s) + 6 HC1(aq) 2 AICI, (aq) + 3 H, (g) > The hydrogen gas produced by this reaction is typically collected via water displacement. During this process, the hydrogen gas becomes saturated with water vapor. If 234.0 mL of gas with a total pressure of 1.03 atm is collected via water displacement at 29.4 °C, what is the partial pressure of the hydrogen gas in the sample? The vapor pressure of water at 29.4 °C is 30.75 torr. PH, atm How many grams of aluminum must have reacted to produce this quantity of hydrogen gas? mass of aluminum: II

Acetylene can be made reacting calcium carbide with water. CaC2 (s)  + 2 H2O (l)  →→ C2H2 (g)   +  Ca(OH)2 (aq)   Assume that you place 2.65 g CaC2 in excess water and collect the acetylene over water.  The volume of the collected gas is 795 mL at 25.0 °C and a barometric pressure of 735.2 mm Hg.  Calculate the percent yield of acetylene.     Note: the vapor pressure of water at 25.0 °C is 23.8 mm Hg.