Question

A handbook lists the value of the Henry's Law constant as 1.400 ✕ 10−3 mol L-1 atm-1 for methane, CH4, dissolved in water at 25°C. Calculate the mole fraction of methane in water at an methane partial pressure of 380. torr.

Answer #1

According to Henry's law, 'At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of gas in equilibrium with that liquid.'

The law can be expressed as,

p = K_{H} x X

where, p is the partial pressure of the gas, K_{H} is
the Henry's law constant and X is the mole fraction.

Here, p = 380 torr = 0.5 atm, as 1 torr = 0.001315 atm

X = p / K_{H}

X = 0.5 / (1.400 x 10^{-3})

X = 357

Therefore the mole fraction of methane in water will be
**357.**

Henry's law constant for CO2 at 38oC is 2.28 x 10–3
mol/L\cdot⋅atm. Calculate the pH of a solution of CO2 at 38oC in
equilibrium with the gas at a partial pressure of 3.20 atm. Assume
that all dissolved CO2 is in the form of carbonic acid (H2CO3). Ka1
= 4.3 x 10–7 and Ka2 = 5.6 x 10–11 for carbonic acid.

The Henry's law constant for O2 in water at 25 °C is
1.25 × 10-5 mol L-1 kPa-1, and the
solubility is 1.5 × 10-3 mol L-1. What is the
partial pressure of O2 under these conditions?

41. Henry's law constant for CO2
at 38°C is 2.28
×10−3 mol / L ·
atm. Calculate the pH of a solution of
CO2 at 38°C in
equilibrium with the gas at a partial pressure of
3.25atm.
A solution of formic acid (HCOOH) has a pH of 2.17. How many
grams of formic acid are there in 100.0 mL of solution? g/100.0
mL

Using Raoult's law for water and Henry's law for nitrogen,
calculate the pressure and gas-phase composition (mole fractions)
in a system containing a liquid that is 1.200 mole% N2
and 98.80 mole% water in equilibrium with nitrogen gas and water
vapor at 50.0°C.
The Henry's law constant for nitrogen in water is recommended by
NIST to be well represented by
kH = 0.000625 exp[1300 (1/T –
1/298.15)] mol N2 / (kg H2O bar), where
T is measured in Kelvin
a)...

The solubility of oxygen, O2, in water is 7.20 ✕ 10−4 mol/L at
0°C when the nitrogen pressure above water is 0.554 atm. Calculate
the solubility of oxygen in water when the partial pressure of
oxygen above water is 1.083 atm at 0°C? The Henry's Law constant
for oxygen is 1.30 ✕ 10−3 mol/ L atm.

The henry's law constant of gaseous methyl bromide
CH3Br is k=0.159 mol/L -atm at 25oC. what
mass of gaseous CH3Br willl dissolve in 225 mL of water
at 25oC and at a CH3Br partial pressure of
250 mm Hg? ( Molar Mass CH3Br=94.93)
please explain
A. 5.23 g
B. 3.40 g
C. 8.49 g
D. 22.1 g
E. 1.12 g

Calculate the concentration of Co2 in rainwater at 25C using
Henry's law. Assume that the water is saturated with air that
contains 350 ppm of CO2. The Henry's law constant for CO2 is
KH=3.4X10-2 MOL/L-ATM at 15C . Express the result in molarity and
ppm. Calculate the concentration of NO in rainwater at 25 C that is
in equlibrium with polluted air where the NO concentration is 10
ppm. The Henry's law constant for No is Kh=2x10-4 mol/l-atm at 25C...

1) Use Henry's law to determine the molar solubility of helium
at a pressure of 1.9 atm and 25 ∘C. Henry’s law constant for helium
gas in water at 25 ∘C is 3.70⋅10−4M/atm.
2) A 2.800×10−2M solution of NaCl in water
is at 20.0∘C. The sample was created by dissolving a sample of NaCl
in water and then bringing the volume up to 1.000 L. It was
determined that the volume of water needed to do this was 999.2 mL...

1. The Henry's law constant for helium gas in water at 30 ∘C is
3.7×10−4M/atm; the constant for N2 at 30 ∘C is
6.0×10−4M/atm.
a. If helium gas is present at 2.1 atm pressure,
calculate the solubility of this gas.
b. If N2 is present at 2.1 atm pressure, calculate
the solubility of this gas.
2. A solution is made containing 14.7 g of CH3OH in 186 g
H2O.
a. Calculate the mass percent of CH3OH.
...

In water at 68°F at sea level (1 atm), water contains about 42
mg/L of dissolved oxygen. Determine the value of Henry's law
constant for oxygen dissolving in water. Recall that air is 21%
oxygen.
A)
6.3 ´ 10–3 mol/(L atm)
B)
0.010 mol/(L atm)
C)
0.25 mol/(L atm)
D)
1.9 ´ 10–2 mol/(L atm)
E)
1.3 ´ 10–3 mol/(L atm)

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