Understanding the high-temperature behavior of nitrogen oxides is essential for controlling pollution generated in automobile engines. the decomposition of nitric oxide (no) to n2 and o2 is second order with a rate constant of 0.0796 m−1⋅s−1 at 737∘c and 0.0815 m−1⋅s−1 at 947∘c. you may want to reference (page) section 14.5 while completing this problem. part a calculate the activation energy for the reaction. express the activation energy in kilojoules per mole to three significant digits.

We have that for the Question "Calculate the activation energy for the reaction" it can be said that The  activation energy is

Ea=1.150KJ/mol

From the question we are told

Understanding the high-temperature behavior of nitrogen oxides is essential for controlling pollution generated in automobile engines. The decomposition of nitric oxide (no) to n2 and o2 is second order with a rate constant of 0.0796 m−1⋅s−1 at 737∘c and 0.0815 m−1⋅s−1 at 947∘cActivation energy

Generally the equation for the Activation energy  is mathematically given as

Ea=1.150KJ/mol

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Van der waals forces are temporary electromagnetic forces established between uncharged atoms. some neutral molecules, when close together, can become temporarily “charged,” as electrons move around the atom. water is a polar molecule, the side of the molecule that the hydrogens bond to being more positive, and the opposite side bound to the lone pairs of electrons being more negative. this means that it participates in dipole-dipole interaction (non-polar exhibits dispersion forces), and it has the capacity for hydrogen bonding.

Moles of co₂ = 2.35/44 = 0.0534 mole.from ideal gas equation pv=nrt,  t = 18+273k = 291 kelvin.∴px5 = 0.0534x0.0821x291∴p = 0.0534x0.0821x291/5 = 0.2551 atm.now, 1 atm = 760 mm of hg  ∴ 0.02551 atm = 0.02551 x 760 = 19.38 mm of hg