A reaction between liquid reactants takes place at [tex]15.0^\circ C[/tex] in a sealed, evacuated vessel with a measured volume of 30.0 L. Measurements show that the reaction produced 38.8 g of carbon monoxide gas. Calculate the pressure of carbon 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.

Using the ideal gas law PV=nRT, the pressure of the carbon monoxide gas in the vessel after the reaction, rounded to two significant figures, is calculated as 1.2 atm.

Explanation:

The subject at hand deals with ideal gas law application, in specific we're calculating the pressure of a gas after a reaction. Given that the temperature T =15.0 °C , which convert to Kelvin it will be 273.15+15.0 = 288.15 K. The volume V is given as 30.0 L and the amount of carbon monoxide produced n, is 38.8 g, which equals to 38.8 g / 28.01 g/mol (molar mass of CO) = 1.385 moles.

The ideal gas law is defined as PV=nRT, where R is the ideal gas constant equal to 0.0821 L•atm/mol•K. By inserting all the values into the formula, we acquire the pressure P:

P = nRT / V = (1.385 mol * 0.0821 L•atm/mol•K * 288.15 K) / 30.0 L = 1.20 atm

So, the pressure of the CO gas in the vessel after the reaction is 1.2 atm, rounded to 2 significant digits.

Learn more about Ideal Gas Law here:

https://brainly.com/question/30458409

#SPJ11