Question

Information:

In this experiment, you will fill a gelatin capsule with an alloy
sample. If the mass of the gelatin capsule is 0.123 g, and the mass
of the capsule plus alloy sample is 0.215 g, calculate the
mass, in grams, of the alloy sample. - 0.092 g |

The
temperature of the water is 24.0 |

A. The barometric pressure is 766.1 mmHg. The vapor pressure of water at 24.0 C is 22.4 mmHg. Calculate the pressure, in mmHg, of the dry hydrogen gas.

B. Convert the pressure of the dry H2 to units of atm. 760.0 mm Hg = 1 atm.

C. Calculate moles of H2 produced in the reaction. R = 0.08206 L atm/(mol K)

Answer #1

A .

According to dalton's law total pressure of gas is equal to sum of partial pressure exerted by each individual gas

P_{total} = P_{1} + P_{2}

P_{H2} = P_{total} - P_{water
vapour}

P_{H2} = 766.1 - 22.4 = 743.7 mmHg

**Pressure of dry hydrogen gas = 743.7 mmHg**

B.

760.0 mmHg = 1 atm then 743.7 mmHg = 743.7 X 1 / 760 = 0.97855 atm

**743.7 mmHg = 0.97855 atm**

C.

Use ideal gas equation for calculation of mole of gas

Ideal gas equation

PV = nRT where, P = atm pressure= 0.97855 atm,

V = volume in Liter = 89.5 ml = 0.0895 L

n = number of mole = ?

R = 0.08206L atm mol^{-1} K^{-1}
=Proportionality constant = gas constant,

T = Temperature in K = 297.15 K

We can write ideal gas equation

n = PV/RT

Substitute the value

n = (0.97855X 0.0895) / (0.08206X 297.15) = 0.00359 mole

**mole of H _{2} produced in reaction = 0.00359
mole**

Q1))) A student carried out this experiment and found:
mass gelatin capsule = (1.2010x10^-1) grams
mass alloy sample + gelatin capsule = (2.86x10^-1) grams
mass empty beaker= (1.4083x10^2) grams
mass beaker + displaced water= (2.9086x10^2) grams
temperature= 294.15 K
Barometric pressure= 746 mmHg
vapor pressure of water= 18.65 mmHg
How many liters of hydrogen gas were produced? Enter answer in
scientific notation with three significant figures.
Q2.))) A student performed this lab, but accidentally used the
barometric pressure in his...

A 0.2755 g sample of an iron-carbon alloy was treated with 12.0
mL of a HCl solution. The alloy sample produced 74.5 mL of H2 gas
at 2 atm and 25.0 oC. Determine the molarity of the HCl solution.
Determine the mass % of iron in the alloy. 2 Fe + 6 HCl T 2 FeCl3 +
3 H2

A 0.250-g sample of a magnesium-aluminum alloy dissolves
completely in an excess of HCl(aq). When the liberated H2(g) is
collected over water at 29 ∘C and 752 torr, the volume is found to
be 345 mL . The vapor pressure of water at 29 ∘C is 30.0 torr. A)
How many moles of H2 can be produced from x grams of Mg in
magnesium-aluminum alloy? The molar mass of Mg is 24.31 g/mol. B)
How many moles of H2 can...

a particular sample of a zinc-aluminum alloy weighs 3.00 g and
has mass percentages of 72.5% Zn and 27.5% Aluminum.
a) How many moles of each element is in the alloy sample?
b) How many theoretical moles of H2(g) will be produced by the
reaction of HCl (aq) with each metal and what will be the total
number of moles produced?
c) How many actual moles of H2(g) will be produced by the
reaction of HCl (aq) with each metal...

For the given data, calculate the masses, pressure, mols, volume
& gas constant R.
DATA -
(M1) Mass of empty capsule = 0.109g
(M2) Mass of capsule filled with sample = 1.501g
(M3) Mass of system before reaction = 100.5g
(M4) Mass of system after reaction = 99.90g
Temp CO2 in celsius = 22
Atmospheric pressure in room = 757
Volume of CO2 = 200ml
Calculate >>>
a) Mass: sample in capsule
b) Mass CO2
c) Pressure CO2 (g) in...

A 0.250-g sample of a magnesium-aluminum alloy dissolves
completely in an excess of HCl(aq). When the liberated H2(g) is
collected over water at 29 ∘C and 752 torr, the volume is found to
be 325 mL . The vapor pressure of water at 29 ∘C is 30.0 torr.
How many moles of H2 can be produced from x grams of Mg
in magnesium-aluminum alloy? The molar mass of Mg is 24.31
g/mol.
Express your answer in terms of x to...

1. A sample of gas with an initial volume of 28.2 L at a
pressure of 728 mmHg and a temperature of 301 K is compressed to a
volume of 14.9 L and warmed to a temperature of 375 K. What is the
final pressure of the gas?
2. A gas sample with a volume of 5.3 L has a pressure of 725
mmHg at 24C. What is the pressure of the sample if the volume
remains at 5.3 L...

1. Hydrogen produced in the following reaction is collected over
water at 23oC and 742 Torr:
2Al + 6HCl --> 2AlCl3 +
3H2
What volume (mL) of the gas will be collected in the reaction of
1.50 g Al with excess HCl?
2. Sample of O2 gas has a volume of 50.0 L at a pressure of 750.
mmHg. What is the final volume, in liters, of the gas at 2.0
atm?
3. What is the mass, in grams, of...

1. Hydrogen produced in the following reaction is collected over
water at 23oC and 742 Torr: 2Al + 6HCl --> 2AlCl3 + 3H2 What
volume (mL) of the gas will be collected in the reaction of 1.50 g
Al with excess HCl?
2. Sample of O2 gas has a volume of 50.0 L at a pressure of 750.
mmHg. What is the final volume, in liters, of the gas at 2.0
atm?
3. What is the mass, in grams, of...

n this exercise, weighed samples of a solid unknown containing
NaCl and NaHCO3 react with hydrochloric acid. The volume of the CO2
liberated by the reaction in the gas phase is measured with a gas
collection syringe. From the volume we can calculate the number of
moles of CO2 in the gas phase using the ideal gas
approximation.
Since the CO2 is generated in an aqueous environment (aqueous
HCl), some CO2 will dissolve in the liquid phase. The amount of...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 2 minutes ago

asked 4 minutes ago

asked 16 minutes ago

asked 18 minutes ago

asked 25 minutes ago

asked 31 minutes ago

asked 43 minutes ago

asked 48 minutes ago

asked 48 minutes ago

asked 52 minutes ago

asked 56 minutes ago

asked 1 hour ago