Please explain and show every step in detail ........

Consider the reaction:

H2 (g) + O2 (g) ⇌ H2O2 (l)             

At 100K 0.345atm hydrogen gas and 0.550atm oxygen gas are initially charged in reaction vessel.  At equilibrium 0.220atm of hydrogen gas remains, calculate Kp for the reaction.

Your answer must include an ICE table, the equilibrium expression and equilibrium reaction.........

Consider the reaction:

2 SO2(g) + O2(g) =2 SO3(g)<-----this is an equilibrium reaction

Kp = 0.355 at950K

A 2.75-L reaction vessel at950K initially contains 0.100 mol of SO2 and 0.100mol of O2. Calculate the total pressure (in atmospheres)in the reaction vessel when equilibrium isreached.

Solid carbon can react with gaseous water to form carbon monoxide gas and hydrogen gas. The equilibrium constant for the reaction at 700.0 K is 1.6×10^−3 Kp .

If a 1.55-L reaction vessel initially contains 195 torr of water at 700.0 K in contact with excess solid carbon, find the percent by mass of hydrogen gas of the gaseous reaction mixture at equilibrium.