Respuesta :
Explanation:
The given data is as follows.
Pressure of moist hydrogen gas = 1.018 atm
Pressure of water vapor = [tex]32 torr \times \frac{1 atm}{760 torr}[/tex]
= 0.0421 atm
Formula to calculate the pressure of dry hydrogen gas is as follows.
Pressure of [tex]H_{2}[/tex] gas = [tex]P_{moist H_{2}} - P_{H_{2}O}[/tex]
Now, putting the given values into the above formula as follows.
Pressure of [tex]H_{2}[/tex] gas = [tex]P_{moist H_{2}} - P_{H_{2}O}[/tex]
= 1.018 atm - 0.0421 atm
= 0.976 atm
Therefore, we can conclude that partial pressure of hydrogen gas in the given sample is 0.976 atm.
Answer:
0.582 g
Explanation:
The vapor pressure of the water = 32 torr
The conversion of P(torr) to P(atm) is shown below:
[tex]P(torr)=\frac {1}{760}\times P(atm)[/tex]
So,
Pressure = 32 / 760 atm = 0.0421 atm
Total pressure = 1.018 atm
Pressure of hydrogen gas = 1.018 - 0.0421 atm = 0.9759 atm
Temperature = 30 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T₁ = (30 + 273.15) K = 303.15 K
Volume = 226 mL = 0.226 L
Using ideal gas equation as:
PV=nRT
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Applying the equation as:
0.9759 atm × 0.226 L = n × 0.0821 L.atm/K.mol × 303.15 K
⇒n = 0.0089 moles
According to the given reaction,
[tex]Zn_{(s)} + 2 HCl_{(aq)}\rightarrow ZnCl_2_{(aq)} + H_2_{(g)}[/tex]
1 mole of hydrogen gas is produced from 1 mole of Zn
0.0089 mole of hydrogen gas is produced from 0.0089 mole of Zn
Thus, Moles of zinc = 0.0089 moles
Molar mass of zinc = 65.39 g/mol
Mass= Moles * Molar mass = 0.0089 * 65.39 g = 0.582 g
