how many grams of sodium are needed to produce 33.2L of hydrogen gas according to the following reaction at 25 degrees celcius and 1 atm?
Sodium(s) + water(l) yields to sodium hydroxide (aq) + hydrogen (g)
1) find the moles of H2 produced
Given:
P = 1.0 atm
V = 33.2 L
T = 25.0 oC
= (25.0+273) K
= 298 K
find number of moles using:
P * V = n*R*T
1 atm * 33.2 L = n * 0.08206 atm.L/mol.K * 298 K
n = 1.357 mol
2)
the balanced chemical reaction is:
2 Na (s) + 2 H2O (l) —> 2 NaOH (aq) + H2 (g)
from reaction,
moles of Na required = 2*moles of H2 produced
= 2*1.357 moles
= 2.714 moles
Molar mass of Na = 22.99 g/mol
mass of Na,
m = number of mol * molar mass
= 2.714 mol * 22.99 g/mol
= 62.4 g
Answer: 62.4 g
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