Chemistry, 19.12.2019 22:31 webbjalia04

Indicate whether each statement is true or false. if you measure the rate constant for a reaction at different temperatures, you can calculate the overall enthalpy change for the reaction. exothermic reactions are faster than endothermic reactions. if you double the temperature for a reaction, you cut the activation energy in half.

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Answer from: gm2

False, False, False

Explanation:

Indicate whether each statement is true or false.

If you measure the rate constant for a reaction at different temperatures, you can calculate the overall enthalpy change for the reaction. FALSE. The relation between the rate constant (k) and the activation energy (Ea) is given by the Arrhenius equation, that is, k depends on the Ea, but not on the enthalpy (ΔH).Exothermic reactions are faster than endothermic reactions. FALSE. Whether a reaction is exothermic or endothermic is defined by the sign of the enthalpy. However, as stated previously, the rate constant (and the rate reaction) do not depend on the enthalpy of the reaction.If you double the temperature for a reaction, you cut the activation energy in half. FALSE. The activation energy does not depend on the temperature.

Answer from: Quest

answer : (a) volume of the gas = 8.67 × $10^{-3}$ l

(b) second virial coefficient b = -1.21226 l/mole

solution : given, t = 300k

p = 20atm

z = 0.86

n = 8.2 mmoles = 8.2 × $10^{-3}$ moles

r = 0.082 l atm/k/mol

find, (a) volume of gas and (b) second virial coefficient b at 300k.

formula used : $z=\frac{pv}{nrt}$

and $z=1+\frac{b}{v}$

(a) $z=\frac{pv}{nrt}$

$v=\frac{znrt}{p}$

= $\frac{0.86\times 8.2\times[tex]10^{-3}$ \times 0.082\times 300}{20}[/tex]

= 8.67 × $10^{-3}$ l

(b) $z=1+\frac{b}{v}$

$b=(z-1)v$

= (0.00867-1) × 8.659

= - 8.5839 l/mole

Answer from: Quest

What do you need with it’s not a question your just stating what it says

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