If ΔG is negative, a reaction is spontaneous in the forward direction. A reaction that is not spontaneous at low temperature can become spontaneous at high temperature if ΔH is ________ and ΔS is ________.
a. -, -
b. +, +
c. +, 0
d. -, +
e. +, -
Which one of the following statements is true about the equilibrium constant for a reaction if ΔG° for the reaction is negative?
a. K = 1
b. K > 1
c. More information is needed.
d. K = 0
e. K < 1
Which element is oxidized in the reaction below?
Fe(CO)5(l) + 2HI(g) Fe(CO)4I2(s) + CO(g) + H2(g)
Which substance is the reducing agent in the reaction below?
Pb + PbO2 + 2H2SO4 2PbSO4 + 2H2O
What is the oxidation state of manganese in manganese dioxide?
What is the coefficient of the permanganate ion when the following equation is correctly balanced?
MnO4- + Br- Mn2+ + Br2 (acidic solution)
The balanced half-reaction in which dichromate ion is reduced to chromium (III) ion is a __________ process.
Which of the following transformations could take place at the cathode of an electrochemical cell?
b. Br2 -> BrO3-
c. HSO4- -> H2SO3
d. Mn2+ _> MnO4-
e. MnO2 -> MnO4-
Answer is (e). For any reaction to be spontaneous free energy should be negative. So for a reaction at low to become spontaneous enthalpy should be +ve and entropy should be -ve to male free energy negative
Answer is ...
The solutions provide answers to a variety of multiple choice questions relating to spontaneous reactions, oxidization, reducing agents, etc.
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