When HNO3 is added to HCN(aq), the CN^- concentration is:
(a) increased (b) decreased (c) not changed
Question # 2
For each of the following processes, state whether nuclear fission, nuclear fusion, or neither fission nor fusion is occurring:
(a) production of energy in the interior of the sun
(b) burning of gasoline
(c) explosion of the atomic bomb at Hiroshima in 1945
(d) production of electricity at the Indian point nuclear power plant
State whether the statements are true or false.
1. If a process is reversible, there is no change in the entropy of the universe.
2. Samples of the same polymer may have different average molecular weights.
3. The half-life of a reagent is the amount of time required for the concentration of that reagent to drop to ½ its original value.
4. For a system at equilibrium, the reaction quotient equals the equilibrium constant.
5. An Arrhenius base generates an excess of OH− ions in solution.
6. A buffer solution is formed by adding a large excess of acid to a solution containing its conjugate base.
7. When a weak acid is titrated against a strong base, the equivalence point occurs at a pH greater than 7.
Q1. When HNO3 is added, we are adding a common ion H+ to the HCN equilibrium HCN ---> H+ + CN- As product is being ...
A number of true/false questions in kinetics and acids and bases are answered.
General High School Chemistry Questions
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1. For each of the following situations, identify those for which a reaction is likely to occur. For those that do occur, write a net ionic equation.
a) A solution of lead(ll) nitrate mixed with a solution of sodium chloride:
b) A solution of sodium sulfate mixed with a solution of calcium chloride:
c) A solution of magnesium acetate mixed with a solution of silver nitrate
2. Explain why you would expect a BeCl2 molecule to be linear but an SCl2 molecule to be angular.
3. Use the standard enthalpies of formation to determine the change in enthalpy for the combustion of methane gas (CH4(g)).
4. In the reaction, H3BO3 + IO3-  HIO3 + H2BO3-, calculate whether the products or the reactants are favored at equilibrium.
5. Calculate the voltage of a standard cell with the following oxidation-reduction reaction.
I2 + Cu  2I- + Cu2+
6. Draw and give the IUPAC name for 5 isomers of C4H7Cl
7. Give structural formulas for the following compounds.
c) Butyl ethanoate
8. Balance the following equations by the half-cell method. Show both half-cell reactions and identify them as oxidation or reduction.
a) SO32- + MnO4- + H+  Mn2+ + SO42- + H2O(l)
b) Cl2(g) + OH-  Cl- + ClO3- + H2O(l)
c) SO42- + I- + H+  S2- + I2(s) + H2O(l)