2 years ago

If you measure the value of Hydronium concentration is 3.0x10^-3 M/L, could you predict the

1 answer:

5 0

pH=-log[H₃O⁺]

pH=- log [3 x 10⁻³]

pH=3-log 3 ⇒ pH<7 = acid

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OverLord2011 [107]

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Viefleur [7K]

Answer:

$\Delta H_{298}^{0}$ for the process is -375 kJ

Explanation:

Summation of change in standard enthalpy ( $\Delta H_{298}^{0}$ )of the two elementary reactions give $\Delta H_{298}^{0}$ of the reaction $P(s)+\frac{5}{2}Cl_{2}(g)\rightarrow PCl_{5}(g)$ .

$P(s)+\frac{3}{2}Cl_{2}(g)\rightarrow PCl_{3}(g)$ ...... $\Delta H_{1}=-287kJ$

$PCl_{3}(g)+Cl_{2}(g)\rightarrow PCl_{5}(g)$ ...... $\Delta H_{2}=-88kJ$

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$P(s)+\frac{5}{2}Cl_{2}(g)\rightarrow PCl_{5}(g)$

$\Delta H_{298}^{0}$ = $\Delta H_{1}+\Delta H_{2}=-287kJ-88kJ=-375kJ$

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