HEN
A 45.2 g sample of Nitrogen gas, N2, has a volume of 3,456mL and a
temperature of 25.0 °C. What is the pressure of the gas? *
F
O 1160 kPa
O 1.15 kPa
O 11.4 kPa
SES
EBRER
96.8 kPa

Pressure of the nitrogen gas is 2290 kPa.

Explanation:

Using the ideal gas equation, we can find the pressure of the gas using the equation as,

PV = nRT

Where P is the pressure = ?

V is the volume = 3,456 ml = 3.456 L

n is the number of moles =  =  = 3.2 mol

R is the gas constant  = 0.08205 L atm  K⁻¹ mol⁻¹

T is the temperature = 25 + 273 = 298 K

Now, rewriting the equation, we will get,

P =

=

= 22.6 atm

Now Pressure in 22.6 atm is converted as 2290 kPa.

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.

ca has a crystalline lattice with positive ions (since it is a metal, metals are positively charged) and electrons flow freely in its structure since the ca atoms have a large nuclear radius so the electrons are not tightly held, therefore the electrons can flow freely since they are not being highly attracted by the nucleus. moreover, one of the properties of metals are that they are conductors of electricity, thus proving ca is the element.