Enter your answer in the provided box. Calculate the volume (in liters) occupied by 2.35 moles of nitric oxide (NO) at 6.18 atm and 63°C.

L

10.5L

Explanation:

The volume in this question can be calculated by using the formula for gas law equation as follows:

PV = nRT

Where;

P = pressure (atm)

V = volume (litres)

n = number of moles (mol)

R = gas law constant (0.0821 Latm/molK)

T = temperature (K)

According to the provided information in this question:

P = 6.18 atm

V = ?

n = 2.35 moles

R = 0.0821 Latm/molK

T = 63°C = 63 + 273 = 336K

Using PV = nRT

V = nRT/P

V = 2.35 × 0.0821 × 336/ 6.18

V = 64.83/6.18

V = 10.49

V = 10.5L

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.