2 years ago

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Chemistry

2 answers:

Dominik [7]2 years ago

7 0

Answer:

$2422 - x002x0$

ser-zykov [4K]2 years ago

7 0

Answer:

Mg + 2 HCl = MgCl2 + H2

2 AgNO3 + K2SO4 = Ag2SO4 + 2 KNO3

Explanation:

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galina1969 [7]

Answer:

$k_2=2.55\ {Ms}^{-1}$

Explanation:

Using the expression,

$\ln \dfrac{k_{1}}{k_{2}} =-\dfrac{E_{a}}{R} \left (\dfrac{1}{T_1}-\dfrac{1}{T_2} \right )$

Where,

$k_1\ is\ the\ rate\ constant\ at\ T_1$

$k_2\ is\ the\ rate\ constant\ at\ T_2$

$E_a$ is the activation energy

R is Gas constant having value = 8.314 J / K mol

$k_2=?$

$k_1=2.57\ {Ms}^{-1}$

$T_1=701\ K$

$T_2=525\ K$

$E_a=1.5\times 10^2\ kJ/mol$

So,

$\ln \:\frac{2.57}{k_2}\:=-\frac{1.5\times \:10^2}{8.314}\times \left(\frac{1}{701}-\frac{1}{525}\right)\:\:$

$k_2=\frac{2.57}{e^{\frac{352}{40796.798}}}=2.55\ {Ms}^{-1}$

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