Stoichiometry
What is the mass in grams of 2.00 moles of NaCl?
116.88 g
Using the ideal gas law, what variable does the letter P represent?
pressure
On a solubility curve for KNO3, if a point at 20°C corresponds to 30 g KNO3 per 100 g water, is a solution with 35 g KNO3 per 100 g water at 20°C saturated, unsaturated, or supersaturated?
supersaturated
According to the Arrhenius definition, what is an acid? What ion increases in aqueous solution?
A substance that increases H+(or H3O+) concentration in water.
Is dissolving ammonium nitrate in water usually endothermic or exothermic?
NH4NO3(s)+heat→NH4+(aq)+NO3−(aq)
endothermic
If 4.0 g of H2 react with excess O2 to form water, how many grams of H2O are produced? (Reaction: 2H2+O2→2H2O) Molar masses: H2 = 2.02 g/mol, H2O = 18.02 g/mol.
35.7 g
A 2.00 L container holds 1.50 mol of an ideal gas at 300 K. Calculate the pressure in atm.
18.5 atm
How does increasing surface area of a solid solute affect the rate of dissolution?
Larger surface area = faster dissolving
Identify the conjugate base of H2PO4−.
Remove one H+:
HPO42−
Define an exothermic reaction in one sentence.
A reaction that releases heat to the surroundings.
Given the reaction 2Al+3Cl2→2AlCl3, how many moles of Cl2 are required to completely react with 1.50 mol Al?
2.25 moles
A sample of gas at 1.00 atm and 300 K is compressed from 4.00 L to 2.00 L. What is the new temperature in K if the number of moles stays constant?
300 K
How does increasing temperature generally affect the solubility of most solid solutes in water?
Solubility increases as temperature increases
Classify each substance as Arrhenius acid, Arrhenius base, Bronsted-Lowry acid, Bronsted-Lowry base, or combinations: (a) HCl (b) NH3 (c) OH−.
a)both types of acid
b)bronsted-Lowry base
c)both types of base
Exothermic, ΔH=−150 kJ
A reaction has a theoretical yield of 25.0 g of product. If the actual yield is 18.5 g, what is the percent yield?
74%
A 2.50 mol sample of an ideal gas occupies 4.00 L at 1.20 atm. If the gas is transferred to a 10.0 L container and heated to 350 K, what is the new pressure of the gas? Assume the initial temperature was 300 K.
0.560 atm
Calculate the molarity of a solution made by dissolving 5.85 g NaCl in enough water to make 0.500 L of solution. (Molar mass NaCl = 58.44 g/mol)
0.200 M
Write the net ionic equation for the neutralization reaction between hydrochloric acid and sodium hydroxide. Hint: Predict the product(s).
H+(aq)+OH−(aq)→H2O(l)
In a calorimetry experiment, 50.0 g of water absorbs 6280 J of heat. Calculate the temperature rise. (Use specific heat of water c=4.184)
ΔT=30.0∘C
Combustion of 3.00 g of propane (C3H8) produces CO2 and H2O. Using the balanced equation C3H8+5O2→3CO2+4H2O, how many moles of CO2 are produced? (Molar mass C3H8C3H8 = 44.10 g/mol)
0.204 mol
A 5.00 L tank contains nitrogen gas at 25.0°C and 4.00 atm. How many grams of N2 are in the tank?
22.9 g
A solution is prepared by dissolving 0.250 mol of solute in 500.0 mL of solution. What is the molarity? Then, if 100.0 mL of this solution is diluted to 500.0 mL, what is the new molarity?
0.100 M
A student mixes 25.0 mL of 0.100 M HCl with 25.0 mL of 0.100 M NaOH. Calculate the concentration of H+ remaining and state whether the final solution is acidic, basic, or neutral.
1.0×10−7 M = Neutral (pH = 7)
A calorimeter contains 100.0 g of water initially at 22.0°C. A 12.0 g metal sample at 95.0°C is placed in the water; the final equilibrium temperature is 24.5°C. Assuming no heat loss and cwater=4.184, calculate the specific heat capacity of the metal.
c=1.24