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

PH2=738 torr×1 atm760 torr

PH2=0.971 atm

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

1 mL = 10-3 L

VH2=160 mL×10-3 L1 mL

VH2=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)

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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.)

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Collecting Gas Over Water concept. If you need more Collecting Gas Over Water practice, you can also practice Collecting Gas Over Water practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Lee's class at UMD.