R = 8.314 J/mol-K = 0.0806 L-atm/mol-K F = 96, 485 C/mol delta G degree = -RT ln

Question

R = 8.314 J/mol-K = 0.0806 L-atm/mol-K F = 96, 485 C/mol delta G degree = -RT ln K delta G = delta G degree + RT ln Q E = E degree - 0.059 V/n log Q at 25 degree C delta G degree = -nFE degree Give the oxidation number of the underlined element in each of the following: (a) S_2O^2-_3 (b) NaH (c) F_2O State whether delta S is positive, negative, or zero for each of the following processes: (a) N_2O(g) reacts with H2(g) at constant temperature and volume to produce NH3(g) (b) 24 g of liquid water freezes to ice at 0 degree C and 1 atm The solubility of Ag_2CO_3 in Na_2CO_3(aq) is (a) the same as its solubility in pure water (b) greater than its solubility in pure water (c) less than its solubility in pure water (a) CuCl_2 (b) Ba(NO_3)_2 (c) AgNO_2 (d) none of these

Explanation / Answer

1)

a)

oxidation state of O is -2

Let oxidation state of S be x

then,

net charge = -2

2*x + 3*(-2) = -2

2x - 6 = -2

2x = 4

x = 2

Answer: +2

b)

Oxidation state of Na is +1

So,

oxidation state of H = -1

c)

Here between F and O, F will be more electronegative

SO,

oxidation state of F is -1

Let oxidation state of O be x

then,

net charge = 0

2*(-1) + x = 0

-2 + x = 0

x = 2

Answer: +2

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