A gaseous sample of nitrogen contains 2.41 grams (0.086 mol). What volume does this mixture occupy at 28 °C and 1.05 atm of pressure? Hint = Be sure to convert to Kelvin first!

0.19 L

0.38 L

1.8 L

2.0 L

4.0 L

2.20L

Explanation:

Number of moles = 0.086moles

Volume = ?

Temperature (T) = 28°C = (28 + 273.15)K = 301.15K

Pressure = 1.05atm

R = 0.082J/mol.K

From ideal gas equation,

PV = nRT

P = pressure of the gas

V = volume

n = number of moles of the gas

R = ideal gas constant

T = temperature of the gas

PV = nRT

V = nRT / P

V = (0.086 × 0.082 × 301.15) / 1.05

V = 2.123 / 1.05

V = 2.02L

Volume of the gas is 2.02L

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.

i believe it is a.) released into

explanation: