Dinitrogen monoxide gas is collected at 19.0 °C in an evacuated flask with a measured volume of 30.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.500 atm . Calculate the mass and number of moles of dinitrogen monoxide gas that were collected. Be sure your answer has the correct number of significant digits.

0.626 moles of dinitrogen monoxide gas was collected, this is 27.6 grams

Explanation:

Step 1: Data given

Temperature of Dinitrogen monoxide gas = 19.0 °C = 292 K

Volume of the flask = 30.0 L

Pressure in the flask = 0.500 atm

Step 2: Calculate moles of Dinitrogen monoxide gas

p*V = n*R*T

⇒with p = the pressure of the gas = 0.500 atm

⇒with V = the volume of the flask = 30.0 L

⇒with n = the number of moles of N2O gas = TO BE DETERMINED

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 292 K

n = (p*V) / (R*T)

n = (0.500 * 30.0) / (0.08206 * 292)

n = 0.626 moles

Step 3: Calculate mass N2O gas

Mass N2O gas = moles N2O * molar mass N2O

Mass N2O = 0.626 moles * 44.013 g/mol

Mass N2O = 27.55 grams ≈ 27.6 grams

0.626 moles of dinitrogen monoxide gas was collected, this is 27.6 grams

answer: mercury

explanation:

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.