For the endothermic formation of sulfuric acid h2o(g) + so3(g) ↔ h2so4(g) the pressure of the system and the temperature of the system would shift the reaction to the left.
1. decreasing, lowering
2. decreasing, raising
3. increasing, raising
4. increasing, lowering

Option (1) is the correct answer.

Explanation:

As per Le Chatelier's principle, any disturbance caused in an equilibrium reaction will tend to shift the equilibrium in a direction away from the disturbance.

For example,

As this given reaction is endothermic in the forward direction and exothermic in the backward direction. Thus, in order to shift the reaction on left side we need to decrease the temperature.

Also, the number of moles are more on reactant side as compared to product side. So, when we decrease the number of moles on reactant side then the equilibrium will shift on left side.

Therefore, we can conclude that for the given reaction decreasing the pressure of the system and lowering the temperature of the system would shift the reaction to the left.

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.

it is the most commonly accepted one