Suppose that 5.14 x 10-3 mol of hydrogen gas occupies a 1,171 ml container at 60°c. what is the pressure (in torr)? (do not type the units.)

Explanation:

Given that:

Temperature = 60 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T₁ = (60 + 273.15) K = 333.15 K  

n = 5.14 × 10⁻³ mol

V = 1,171 mL = 1.171 L ( 1 mL = 0.001 L)

Using ideal gas equation as:

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 62.364 L Torr/ K mol  

Applying the equation as:

P × 1.171 L = 5.14 × 10⁻³ mol × 62.364 L Torr/ K mol  × 333.15 K  

⇒P = 91.2 torr

it should be p1 v1 = p2 v2

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.