What is the mass of neon that exerts a pressure of 720. mmhg, with a temperature of -15.0 °c , when the volume of the container is 760. ml?

Mass = 0.61 g

Explanation:

Given data:

Pressure of neon gas = 720 mmHg

Temperature = -15.0°C

Volume = 760 mL

Mass of neon gas = ?

Solution:

720 mmHg = 720/760 = 0.95 atm

-15.0°C + 273 = 258 K

760/1000 = 0.76 L

PV = nRT

n = PV/RT

n = 0.95 atm ×0.76 L/ 0.0821 atm. L. k⁻¹.mol⁻¹× 258 K

n = 0.722 atm. L/ 21.2 atm. L. mol⁻¹

n = 0.03 mol

Mass of neon:

Mass = number of moles × molar mass

Mass = 0.03 mol × 20.2 g/mol

Mass = 0.61 g

that tool would be a compass

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.