Equilibrium and Le Chateleir's Principal
Instructions: Write the equilibrium expression for each chemical equation.
Oxidation-Reduction Reactions
Instructions: Assign an oxidation state to each element, ion, or molecule.
Instructions: Assign an oxidation state to each atom in each compound.
Instructions: Assign an oxidation state to each atom in each polyatomic ion.
Instructions: Identify the oxidation state of P in each ion.
i) 2 H2S(g) ====== 2H2(g) + S2(g)
Keq = [H2(g)]^2*[S2(g)]/[H2S(g)]^2
ii) NH4HS(S) ======= NH3(g) + H2S(g)
Keq = [NH3(g)]* [H2S(g)]
iii) oxidation state Cl in Cl- is -1
oxidation state of Br in Br2 is 0
oxidation state of K is 0
oxidation state of Ca in Ca2+ is +2
iv) In NaCl oxidation state of Na is +1 and that of Cl is -1
In CH4 oxidation state of C is -4 and that of H is +1
In SbCl5 oxidation state of Sb is +5 and that of Cl is -1
In Al2O3 oxidation state of Al is +3 and that of O is -2
v) In NH4+ oxidation state of N is -3 and that of H is +1
In ClO4- oxidation state of Cl is +7 and that of O is -2
In Cr2O7 2- oxidation state of Cr is +6 and that of O is -2
In MnO4- oxidation state of Mn is +7 and that of O is -2
vi) In PO43- oxidation state of P is +5
In HPO42- it is +5
In H2PO4- it is +5
In H3PO4 it is +5
Equilibrium and Le Chateleir's Principal Instructions: Write the equilibrium expression for each chemical equation. 2 H2Sg⇌2H2g+S2g...
For the following reaction, calculate how many moles of NO2 forms when 0.356 moles of the reactant completely reacts. 2 N2O5g→4 NO2g+O2g For the following reaction, calculate how many moles of each product are formed when 0.356 moles of PbS completely react. Assume there is an excess of oxygen. 2PbSs+3O2g→2PbOs+2SO2g For the following reaction, calculate how many grams of each product are formed when 4.05 g of water is used. 2 H2O→2 H2+O2 4. Determine the theoretical yield of P2O5,...
Equilibrium and Le Chateleir's Principal Instructions: Write the equilibrium expression for each chemical equation. 1. 2 H = 2H26) +S260) 1.65 X 10 -7 at 1070 K 2. NH4HS(s) + NH3q + H2S(g) 1.33X10 -5 at 257 K
Write an expression for the equilibrium constant of each chemical equation. SbCl5(g)⇌SbCl3(g)+Cl2(g)SbCl5(g)⇌SbCl3(g)+Cl2(g) 2 BrNO (g)⇌2 NO(g)+Br2(g)2 BrNO (g)⇌2 NO(g)+Br2(g) CH4(g)+2 H2S(g)⇌CS2(g)+4 H2(g)CH4(g)+2 H2S(g)⇌CS2(g)+4 H2(g) 2 CO(g)+O2(g)⇌2 CO2(g)