The volume of hydrogen gas at 38 degree C and 763 torr that can be produced by the reaction of 4.33g of zinc?

Question

The volume of hydrogen gas at 38 degree C and 763 torr that can be produced by the reaction of 4.33g of zinc with excess sulfuric acid is _________L.

Zn + H2SO4  H2 + ZnSO4

Answer 1

First, find the moles of gas from the starting materials & balanced equation, then you can calculate the volume with the ideal gas law.

The ratio from the equation is 1:1 and it was specified the sulfuric acid was in excess so moles of zinc = moles of hydrogen.

4.33g/65.37g/mole = 0.0662mole

Now use the gas equation:

PV = nRT solve for V: V = nRT/P

0.0662mole x 0.08206Latm/moleK x 311K/1.004 atm = 1.68liters

Answer 2

in accordance to what i discover, hydrogen isn't a made from the detonation of TNT: The equation is: Upon detonation, TNT decomposes as follows: 2 C7H5N3O6 ? 3 N2 + 5 H2O + 7 CO + 7 C Are you helpful that the question is actual - perhaps it asks for quantity of N2. Hydrogen very merely combines with oxygen to produce water. it variety of feels relatively unlikely that there may well be any unfastened hydrogen produced consequently of the detonation of TNT.

Answer 3

Moles Zn = 4.33 g / 65.39 = 0.0662
The ratio between Zn and H2 is 1 : 1 so we would get 0.0662 mole H2
p = 763 / 760 = 1.0 atm
T = 38 + 273 = 311 K
V = nRT / p = 0.0662 x 0.0821 x 311 / 1 = 1.69 L