Calculate the no. of moles of H2 using the ideal gas equation:
• PH2 = 738 torr (atm is needed in the ideal gas equation: convert from mmHg to atm)
1 atm = 760 torr
• V = 160 mL (L is needed in the ideal gas equation: convert from mL to L)
1 mL = 10-3 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 (L∙atm)/(mol∙K)
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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