At a pressure of 101.3 kilopascal and a temperature of 373 k, heat is removed from a sample of water vapor, causing the sample to change from the gaseous phase to the liquid phase. this phase change is represented by the equation h20(g) -> h20(l) + heat. determine the total amount of heat released by 5.00 grams of water vapor during the phase change shown in the given experiment
a catalyst doesn't change the relative energies of reactants and products
a catalyst speeds up a reaction by providing an alternate pathway with a lower activation energy (see image).
more molecules will have enough energy to get over the energy barrier, and the product is formed faster.
a catalyst does not change the energies of the reactants, so it does not change the amount of product at equilibrium.
thus, if the end of the reaction (equilibrium) is reached quickly, a catalyst does not affect the amount of product.
if an uncatalyzed reaction takes a long time (say, a hundred years), then the addition of a catalyst will cause more product to be formed during a laboratory period, but it won't affect the amount formed at equilibrium.
answer: - c. h
explanations: - reduction is gain of electron. in other words we could say that decrease in oxidation number is reduction.
as per the rules, oxidation number of hydrogen in its compounds is +1(except metal hydrides) and the oxidation number of oxygen in its compounds is -2.
the oxidation number in elemental form is zero.
in , the oxidation number of h is +1 and oxidation number of o is -2. oxidation number of cl in is -1. on product side, the oxidation number of hydrogen in is zero and in the oxidation number of h is +1 and that of o is -2. oxidation number of cl in is 0.
from above data, oxidation number of o is -2 on both sides so it is not reduced.
oxidation number of cl is changing from -1 to 0 which is oxidation.
oxidation number of h is changing from +1 to 0 which is reduction.
so, the right choice is c.h