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Zinc reacts with aqueous sulfuric acid to form hydrogen gas: zn(s) + h2so4(aq) → znso4(aq) + h2(g) in an experiment, 201 ml of wet h2 is collected over water at 27°c and a barometric pressure of 733 torr. the vapor pressure of water at 27°c is 26.74 torr. the partial pressure of hydrogen in this experiment is ________ atm.

Respuesta :

The partial pressure of hydrogen = barometric pressure - the vapor pressure of water;
= 733 - 26.74 
= 706.26 torr
But 1 atm is equivalent to 760 torr
Therefore, = 706.26/760
                  = 0.929 atm
Hence, the partial pressure of hydrogen is 0.929 atm

Answer: 0.93 atm

Explanation:

According to Dalton's law, the total pressure of a mixture of gases is the sum of individual pressures exerted by the constituent gases.

[tex]p_{total}=p_A+p_B[/tex]

Thus [tex]p_{total}=p_{H_2O}+p_{H_2}[/tex]

Given: [tex]p_{total}=733torr[/tex]

[tex]p_{H_2O}=26.74torr[/tex]

[tex]p_{H_2}=?[/tex]

Thus [tex]733torr=26.74torr+p_{H_2}[/tex]

[tex]p_{H_2}=706.26torr[/tex]

also 760 torr = 1atm

Thus [tex]706.26torr=\frac{1}{760}\times 706.26=0.93atm[/tex]

Thus the partial pressure of hydrogen in this experiment is 0.93 atm.

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