The equation for the combustion of ethanol is: c2hsoh(i)+302(g) 2c02(g) +3h20(i) given (in kj mol2): = +347 e(c-c) e(c-h) e(c-o e(0=0) e(c o) e(o-h) = +410 = +336 +496 +805 +465 calculate the enthalpy change of the above reaction. (a) the standard enthalpy change of combustion of ethanol is-1367.3 kj mol1. (b) suggest why this value differs from the value obtained using bond energies.

What method(s) do plants use to obtain nitrogen? select all that apply. absorb it from the atmosphere use bacteria to convert nitrogen to usable form obtain usable nitrogen compounds from the soil absorb nitrogen from water taken in at the roots

Liquid ammonia is produced at high temperatures and under great pressure in a tank by passing a mixture of nitrogen gas and hydrogen gas over an iron catalyst. the reaction is represented by the following equation. n2(g) + 3h2(g) → 2nh3(g) changing all but one experimental condition will affect the amount of ammonia produced. that condition is a) increasing the concentration of both reactants b) changing the temperature within the tank c) decreasing the pressure within the tank. d) increasing only the amount of nitrogen present.

Why is any chemical reaction always balanced? give reasons and explain the easiest way to solve the balancing problems in chemical equations with stoichiometric coefficients upto 20 as hit and trial doesn't always work. give full reasoning