When 50.0 mL of 0.100 M AgNO3 is combined with 50.0 mL of 0.100 M HCl in a container, how many moles of AgCl are produced?

Suppose that 0.79 g of water condenses on a 95.0-g block of copper that is initially at 23 °C. If the heat released during condensation goes only to warming the copper block, what is the final temperature (in °C) of the copper block? Assume a constant specific heat capacity for copper.

Suppose that 0.95 g of water condenses on a 75.0 g block of iron that is initially at 22°C. If the heat released during condensation is used only to warm the iron block, what is the final temperature (in °C) of the iron block? (Assume a constant enthalpy of vaporization for water of 2260 J/g and specific heat capacity of iron as 0.449 J/g°C.)

Suppose that 1.08 g of rubbing alcohol (C3H8O) evaporates from a 74.0 g aluminum block. If the aluminum block is initially at 25 °C, what is the final temperature of the block after the evaporation of the alcohol? Assume that the heat required for the evaporation is absorbed entirely from the aluminum block, and the heat of vaporization of rubbing alcohol is 45.4 kJ/mol. The specific heat capacity of aluminum is 0.897 J/g°C.

In the reaction AgNO3(aq) + HBr(aq) → AgBr(s) + HNO3(aq), when 50.0 mL of 4.00×10⁻² M AgNO3 is combined with 50.0 mL of 4.00×10⁻² M HBr, what is the precipitate formed?

The addition of hydroiodic acid to a silver nitrate solution precipitates silver iodide according to the reaction: AgNO3(aq) + HI(aq) → AgI(s) + HNO3(aq). When 50.0 mL of 5.00 × 10^-2 M AgNO3 is combined with 50.0 mL of 5.00 × 10^-2 M HI, what is the mass of silver iodide precipitated?

The heat of vaporization of liquid isopropyl alcohol is 159 cal/g. Calculate the energy required to vaporize 39.5 g of this compound.

The heat of vaporization of water at 100°C is 40.66 kJ/mol. Calculate the quantity of heat that is absorbed or released when 20.00 g of steam condenses to liquid water at 100°C.

The reaction NO2(g) + CO(g) → NO(g) + CO2(g) occurs in one step with an activation energy of 132 kJ/mol and a ΔE of -226 kJ/mol. Is this reaction endothermic or exothermic?