# Problem: Hydrogen gas is produced when zinc reacts with sulfuric acid:Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)If 160 mL of wet H2 is collected over water at 24 oC and a barometric pressure of 738 torr, how many grams of Zn have been consumed? (The vapor pressure of water is 22.38 torr.)

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###### FREE Expert Solution

Calculate the no. of moles of H2 using the ideal gas equation:

Given:

• PH2 = 738 torr     (atm is needed in the ideal gas equation: convert from mmHg to atm)

1 atm = 760 torr

${\mathbit{P}}_{{\mathbf{H}}_{\mathbf{2}}}\mathbf{=}$0.971 atm

• V = 160 mL                (is needed in the ideal gas equation: convert from mL to L)

1 mL = 10-3 L

${\mathbit{V}}_{{\mathbf{H}}_{\mathbf{2}}}\mathbf{=}$0.160 L

T = 24.0°C              ­(K is need in the ideal gas equation: convert from °C to K)

T = 24.0°C + 273.15
T = 297.15 K

R = gas constant = 0.08206 (Latm)/(molK)

###### Problem Details

Hydrogen gas is produced when zinc reacts with sulfuric acid:
Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)

If 160 mL of wet H2 is collected over water at 24 oC and a barometric pressure of 738 torr, how many grams of Zn have been consumed? (The vapor pressure of water is 22.38 torr.)