If you have 5.8x10^23 atoms of tin how many liters of hydrogen gas can you make at 1.0 atm and 25C.

Question

Sn + 4 HNO3 ---> Sn(NO3)4 + 2 H2

Answer 1

Sn + 4HNO₃ ===> Sn(NO₃)₄ + 2H₂ ... balanced equation

moles of Sn present = 5.8x10²³ atoms x 1 mole/6.022x10²³ atoms = 0.96 moles Sn

moles of H₂ gas produced = 0.96 moles Sn x 2 moles H₂ / 1 mol Sn = 1.92 moles H₂

Use the ideal gas law to find the volume of H₂ gas:

PV = nRT

P = pressure = 1.0 atm

V = volume in L = ?

n = moles = 1.92

R = gas constant = 0.0821 Latm/Kmol

T = temperature in K = 25 + 273 = 298K

V = nRT/P = (1.92 mol)(0.0821 Latm/Kmol)(298K) / 1.0 atm

V = 47 liters (2 significant figures)