A piece of sodium metal undergoes complete reaction with water as follows?

Question

2Na(s) + 2H2O(l) -----> 2NaOH(aq) + H2(g)

the hydrogen gas generated is collected over water at 25.0(degree)C. The volume of the gas is 246mL measured at 1.00atm.Calculate the number of grams of sodium used in the reaction.(Vapor pressure of water at 25degree C = 0.0313atm)

Answer 1

sodium is a very reactive metal it react very fast with water and reaction is also very explosive. Because of fast reaction sodium react with water until it consume completely.

Answer 2

The number of H2 molecules is half of the number of Na- atoms.

So N= (p- pv)*V/RT=(1.05 -0.031)*10^5 J/m³  *0.246*10^-3 m³/8.314J/molK*298K=0.0101 mol H2

=> n(Na)= 0.0202 mol

M(Na)= 23 g/mol => m(Na)= 0.4654 g

Answer 3

.246 (1-.0313) = n (.0821) (298)

n Hydrogen = 102.66

2 moles Sodium per Hydrogen

n Sodium = 205.32

g Sodium = 4720.3069