What is the volume of 45.0 grams of nitrogen monoxide , no
at20 degrees celsius and a pressure of 740 mm hg?

Explanation:

Given that:

Mass of , m = 45.0 g

Molar mass of , M = 30.01 g/mol

Temperature = 20.0 °C

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

T(K) = T( °C) + 273.15  

So,  

T₁ = (20.0 + 273.15) K = 293.15 K

V = ?

Pressure = 740 mm Hg

Considering,  

Using ideal gas equation as:

where,  

P is the pressure

V is the volume

m is the mass of the gas

M is the molar mass of the gas

T is the temperature  

R is Gas constant having value = 62.36367 L. mmHg/K. mol

Applying the values in the above equation as:-

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g

it's filtration, but this is an assumption so my apologies if i got this