Question

Liquid Halothane has a density of 1.87 g/mL, and boils at 50.2 degrees celsius and 1.00 atm.

A) If Halothane behaved as an ideal gas, what volume would 10.0 mL of Halothane occupy at 60 degrees celsius and 1.00 atm of pressure? (In Liters)

B) What is the density in g/L of Halothane vapor at 55 degrees celsius and 1.00 atm of pressure?

Answer #1

At temperatures >50.2, Halothane is gas. Hence

From Gas law V= nRT/P, n=number of moles , R=0.08206 L.atm/mole.k, T=60deg.c =60+273.15 =333.15 k

P= 1ATM

Mass of halothanew= Volume*density= 10*1.87= 18.7 gm

Molecular weight of halothane= 197.381

Moles =Mass/Molecular weight =18.7/197.381=0.094

VOLUME =0.094*0.08206*333.15/1 L=2.56 L

B) AT 55 deg.c, from gas law PV= nRT= (Mass/ Molecular weight)*R*T

P * Molecular weight = (Mass/Volume)*RT= density*RT

density = P* Molecular weight/ RT= 1*197.381/ (0.08206*(55+273.15) gm/L=7.32 g/L

The vaporization of 1 mole of liquid water (the system) at 100.9
degrees C, 1.00 atm, is endothermic.
H2O(l) + 40.7kJ ---> H2O (g)
Assume at exactly 100.0 degrees C and 1.00 atm total pressure,
1.00 mole of liquid water and 1.00 mole of water vapor occupy 18.80
mL and 30.62 L, respectively.
1. Calculate the work done on or by the system when 3.65 mol of
liquid H2O vaporizes. Answer in J
2. Calculate the water's change in internal...

What is the density of Xe gas at 0.00 degrees Celsius, at a
pressure of 563 Torr, with volume 36.0 mL?
A). 1.58 g/L
B). 4.99 g/L
C). 2.15 g/L
D). 5.22 g/L
E). 4.34 g/L

A
250 mL container of a gas is at 100 degrees Celsius. At what
temperature will the gas occupy a volume of 125 mL, the pressure
remaining constant?

A gas occupies 40.0 mL at 127 degrees Celsius. What
volume will it occupy at-73 degrees celsius? (Assume pressure and
number of particles is constant.)
A)23.0 ml
B)8.80 ml
C) 79.2ml
D)20.0ml
E) None

Consider the combustion reaction between 25.0mL of liquid
methanol (density=0.850g/mL) and 12.5 L of oxygen gas measured at
STP. The products of the reaction are CO2(g) and H2O(g). Calculate
the volume of liquid H2O (density= 1g/mL) formed if the reaction
goes to completion and you condense the water vapor. *assume that
oxygen is an ideal gas*

Assume at exactly 100.0°C and 1.00 atm total pressure, 1.00 mole
of liquid water and 1.00 mole of water vapor occupy 18.80 mL and
30.62 L, respectively. 1)Calculate the work done on or by the
system when 3.65 mol of liquid H2O vaporizes. 2.)Calculate the
water's change in internal energy

If 1.00 mL of water is placed in a 5.00 L closed flask at 26°C,
what volume of water would remain as liquid after equilibrium is
allowed to establish between the liquid water and the water vapor
in the flask ? (The vapor pressure of water at 26°C is 25.2 torr,
and the density of water at 26°C is 1.00 g/mL.)

The vaporization of 1 mole of liquid water (the system) at
100.9°C, 1.00 atm, is endothermic. $$ Assume that at exactly
100.0°C and 1.00 atm total pressure, 1.00 mole of liquid water and
1.00 mole of water vapor occupy 18.80 mL and 30.62 L,
respectively.
Calculate the work done on or by the system when 4.65 mol of
liquid H2O vaporizes.

1.ethyl chloride is sold as a liquid under pressure for the use
as a local skin anesthetic. ethyl cholride boils at 12 degree
celsius at atmospheric pressure. When the liquid is sprayed onto
skin, it boils off, cooling and numbing the skin as it
vaporizes.
a. what charges at state are involved in this use of ethyl
chloride
b. what is the boling point of cholride in degrees
fahrenheit
c. a bottle contains 103.5 ml ethyl chloride. the denisty of...

When 0.854 g of impure zinc reacted with an excess of
hydrochloric acid, 244 mL of hydrogen gas was collected over water
at 10.0 °C. The external pressure was 714.96 Torr. The vapor
pressure of water at various temperatures can be found in this
table.
a. Calculate the volume the dry hydrogen would occupy at 1.00
atm and 298 K.
b. What amount, in moles, of H2 gas was collected at 10.0
°C?
c.Calculate the percentage purity of the zinc...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 11 minutes ago

asked 11 minutes ago

asked 13 minutes ago

asked 16 minutes ago

asked 35 minutes ago

asked 42 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago