Question

Calculate the molar fraction of nitrogen gas, N_{2},(g)
which is dissolved in water at sea level. The molar fraction
N_{2} (g) in air at sea level is 0.78. Assume that nitrogen
gas behaves as an ideal gas under these conditions.

Answer #1

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)...

20 g of fructose (look up molar mass) is dissolved in 500 g of
water. Calculate the boiling point
of this mixture.

Calculate the volume occupied by 84.0 g of nitrogen gas under
STP
conditions.

A flue gas consists of carbon dioxide, oxygen, water vapor, and
nitrogen. The molar fractions of CO, and 0, in a sample of the gas
are 12% and 6%, respectively. The weight fraction of H,O in the gas
is 6.17%. Estimate the density of this gas at 500 K and 110
kPa.

Hydrazine, N2H4, may react with oxygen to form nitrogen gas and
water. N2H4(aq) + O2(g)→N2(g) + 2H2O(l). If 2.05 g of N2H4 reacts
and produces 0.750 L of N2, at 295 K and 1.00 atm, what is the
percent yield of the reaction?

16.177 g of a non-volatile solute is dissolved in 290.0 g of
water. The solute does not react with water nor dissociate in
solution. Assume that the resulting solution displays ideal
Raoult's law behaviour. At 40°C the vapour pressure of the solution
is 54.506 torr. The vapour pressure of pure water at 40°C is 55.324
torr. Calculate the molar mass of the solute (g/mol).
Now suppose, instead, that 16.177 g of a volatile solute is
dissolved in 290.0 g of...

Hydrazine,
N2H4, may react with oxygen to form nitrogen
gas and water.
N2H4(aq)+O2(g)⟶N2(g)+2H2O(l)
If 3.15 g of
N2H4 reacts and produces 0.750 L of
N2, at 295 K and 1.00 atm, what is the percent yield of
the reaction?
%

Chemistry - Gas Laws:
A 1.00 liter vessel contains 5.00 grams of nitrogen (N2) and
1.50 grams of water at 25°C.
a)Determine the RMS speed of nitrogen molecules and water
molecules in the vapor phase at 25°C.
b)Calculate the average kinetic energyper moleculeof nitrogen
and of water vapor at 25°C.
(Show all work and calculations, include units in
answer. If calculations must be used in several parts, rounding
should be made to 6 decimal points to ensure accuracy. Final
Answers...

1.20 g of MgCO3 are dissolved in water and brought to a final
volume of 700 mL. What is the molar concentration of the
solution?
2.Calculate the normality of the solution.
3. If the MgCO3 completely dissociates to Mg2+ and CO3 2- , what
are the concentrations of Mg2+ and CO3 2- (in g/L) in the
solution?
4. Calculate the mass fraction of Mg2+ in the solution.
5. Calculate the molar fraction of C in solution.

If 100 g of air consists of 77% by weight of nitrogen (N2,
molecular weight = 28), and 23% by weight of oxygen (O2, molecular
weight = 32), calculate (a) the mean molecular weight of air, (b)
mole fraction of oxygen, (c) concentration of oxygen in mol/m3 and
kg/m3, if the total pressure is 1.5 atm and the temperature is
25°C.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 11 minutes ago

asked 22 minutes ago

asked 36 minutes ago

asked 38 minutes ago

asked 50 minutes ago

asked 58 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago