Question
What are significant figures? State rules to determine it.
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Answer
SELF
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- Calculate the $\Delta_\text{r}\text{H}^\circ$ for the reaction:
H2(g) + Br2(g) → 2HBr(g)
Bond enthalpy are given as, H-H = 436kJ mol-1, Br-Br = 192kJ mol-1 and H-Br = 368kJ mol-1
Write a relation between $\triangle G$ and Q and define the meaning of each term and answer the following:
a. Why a reaction proceeds forward when $Q < K$ and no net reaction occurs when $Q = K$.
b. Explain the effect of an increase in pressure in terms of reaction quotient Q for the reaction:
$
CO(g)+3 H_2(g) \rightleftharpoons CH_4(g)+H_2 O(g)
$
→a. Why a reaction proceeds forward when $Q < K$ and no net reaction occurs when $Q = K$.
b. Explain the effect of an increase in pressure in terms of reaction quotient Q for the reaction:
$
CO(g)+3 H_2(g) \rightleftharpoons CH_4(g)+H_2 O(g)
$
What is mole concept? What is relation with molar mass of substance and number of molecule.
The equilibrium constant for the following reaction is 1.6 ×105 at 1024K $\text{H}_2\text{ (g) + Br (g)}\rightleftharpoons2\text{HBr (g)}$ Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a
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→sealed container at 1024K.
Compare the acidic properties of alkane, alkene and alkyne and write reaction to represent the acidic nature of 1-alkyne.
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Why is benzene extra ordinarily stable though it contains three double bonds?
One of the reaction that takes place in producing steel from iron ore is the
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$\text{FeO (S) + CO (g)}\rightleftharpoons\text{Fe (S) + CO}_2\text{ (g)};\text{ K}_{\text{p}}=0.265\text{atm at}1050\text{K}$
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→reduction of iron(II) oxide by carbon monoxide to give iron metal and CO2.
$\text{FeO (S) + CO (g)}\rightleftharpoons\text{Fe (S) + CO}_2\text{ (g)};\text{ K}_{\text{p}}=0.265\text{atm at}1050\text{K}$
What are the equilibrium partial pressures of CO and CO2 at 1050 K if the initial partial pressures are: pCO= 1.4atm and = 0.80atm?
Write the expression for the equilibrium constant, $K _{ c }$ for each of the following reactions :
(i) $2 NOCl ( g ) \rightleftharpoons 2 NO ( g )+ Cl _2(g)$
(ii) $2 Cu \left( NO _3\right)_2(s) \rightleftharpoons 2 CuO ( s )+4 NO _2(g)+ O _2(g)$
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(v) $I _2(s)+5 F_2(g) \rightleftharpoons 2 IF _5$
→(i) $2 NOCl ( g ) \rightleftharpoons 2 NO ( g )+ Cl _2(g)$
(ii) $2 Cu \left( NO _3\right)_2(s) \rightleftharpoons 2 CuO ( s )+4 NO _2(g)+ O _2(g)$
(iii) $CH _3 COOC _2 H _5( aq )+ H _2 O ( l ) \rightleftharpoons$$CH _3 COOH ( aq )+ C _2 H _5 OH ( aq )$
(iv) $Fe ^{3+}( aq )+3 OH ^{-}( aq ) \rightleftharpoons Fe ( OH )_3(s)$
(v) $I _2(s)+5 F_2(g) \rightleftharpoons 2 IF _5$