Chemistry I Final Exam Review

A piece of metal weighing 59.047 g was heated to 100ºC and then put into 100 mL of water (initially at 23.7ºC). The metal and water were allowed to an equilibrium temperature, determined to be 27.8ºC. Assuming no heat lost to the environment, calculate the specific heat of the metal. Specific Heat of water = 4.18J/gºC Density of water = 1.00g/mL

In an experiment, 700 mL of 0.5 M hydrochloride acid (HCl) is added to 600 mL of of 0.5 M sodium hydroxide (NaOH) solution. The acid and base neutralize each other according to the equation: HCl + NaOH --> NaCl + H2O
How many moles of acid and base were there originally?

A chemist wants to determine the enthalpy of neutralization for the following reaction: HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O (l)

The chemist uses a coffee-cup calorimeter to neutralize completely 70.5 mL of 2.56 M HCl (aq) with 30.5 mL of 2.56 M NaOH (aq). The initial temperature of both solutions is 16.8ºC. After neutralization, the highest recorded temperature is 22.6ºC. Calculate the enthalpy of neutralization in kJ/mol of H2O.
Assume that the density of the solution is 1.00 g/mL and specific heat is 4.18 J/gºC

Use the periodic table to predict which element has the largest ionization energy.

Use the periodic table to predict which element has the largest atomic radius.

Which of the following is a transition element?

The element germanium (Ge) is used in the manufacture of some transistors. What other element might be used for such a purpose?

When the excess of calcium carbonate is added to dilute HCl, the reaction gradually becomes slower and finally stops. Which statement best explains why this happens?

The molar volume of a gas-

In the reaction CH4 (g) + 2O2 (g) --> CO2 (g) + 2H2O (g)
18 L of oxygen would produce how many L of CO2 at STP?
(Hint: You must first balance the equation.)

A metal was found to release -1246 J of energy in a calorimeter. Initial temperature was 40.0ºC and the final temperature was 2.00ºC. The specific heat of the metal is 3.14 J/gºC, what is the mass of the metal used?

What is the mass in grams of 17.0 liters of methane gas (CH4) at STP?
MM of CH4 = 16.04 g/mol

During a Carbonate Analysis experiment, a 0.306 g sample of a CaCO3 "mixture" was used to collect 0.061 g CO2. Determine the mass of CaCo3 in the original mixture.
CaCO3 (g) + 2H3O+ (aq) --> Ca2+ (aq) + 2H2O (l) + CO2 (g)
MM of CaCO3 = 100.09 g/mol
MM of Co2 = 44.01 g/mol

A 3 M HCl solution was used to generate the CO2 from the CaCO3 mixture. What would be the effect on the calculations if 6 M HCl was substituted for the 3 M HCl?

Electrons are lost by the-

Phenolphthalein is ______ in basic solutions but _____ in acidic solutions.

In a titration, 34.12 mL of HCl required 42.03 mL of a 0.9981 M NaOH solution to reach the endpoint. Calculate moles of NaOH dispensed.

What is the difference between the endpoint and stoichiometric point in a strong acid/base titration?

At 16.7 mL volume of a 0.0861 M NaOH solution neutralizes 20.0 mL of HCl acid. What is the molar concentration of the HCl solution?