A reaction between liquid reactants takes place at in a sealed, evacuated vessel with a measured volume of . Measurements show that the reaction produced of dinitrogen monoxide gas. Calculate the pressure of dinitrogen monoxide gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to significant digits.

This question is incomplete, the complete question;

A reaction between liquid reactants takes place at 16°C in a sealed, evacuated vessel with a measured volume of 10.0 L . Measurements show that the reaction produced 37.g of dinitrogen monoxide gas.

Calculate the pressure of dinitrogen monoxide gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits.

Explanation:

Given that;

Volume = 10.0 L

Temperature T = 16°C = ( 16 + 273) = 289 K

we know that  molar mass of N₂O = 44 g/mol

number number of moles n will be: weight/molar mass = 37/44 = 0.8409 moles

Universal Gas constant R = 0.0821 atm.mol⁻¹.k⁻¹

pressure p = ?

from the ideal gas law

PV = nRT

P = nRT / n

so we substitute

P = (0.8409 mole × 0.0821 atm.mol⁻¹.k⁻¹ × 289 K) / 10.0 l

P = 19.95195 / 10.0

P = 1.9952 atm

answer

i think the answer is a) as air pressure in an area increases, the density of the gas particles in that area decreases.

hope it