The arrhenius equation shows the relationship between the rate constant k and the temperature t in kelvins and is typically written as k=ae−ea/rt where r is the gas constant (8.314 j/mol⋅k), a is a constant called the frequency factor, and ea is the activation energy for the reaction. however, a more practical form of this equation is lnk2k1=ear(1t1−1t2) which is mathematically equivalent to lnk1k2=ear(1t2−1t1) where k1 and k2 are the rate constants for a single reaction at two different absolute temperatures (t1 and t2). part a the activation energy of a certain reaction is 45.6 kj/mol . at 30 ∘c , the rate constant is 0.0160s−1 . at what temperature in degrees celsius would this reaction go twice as fast

T = 42.08  °C

Explanation:

Using the expression,

Wherem  

is the activation energy

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

Thus, given that, = 45.6 kJ/mol = 45600 J/mol (As 1 kJ = 1000 J)

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (30 + 273.15) K = 303.15 K  

So,

Conversion to °C as:

T(K) = T( °C) + 273.15  

So,  

315.23 = T( °C) + 273.15

T = 42.08  °C

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.