We can use the ideal gas law equation to find the number of moles in the gas
PV = nRTwhere P - pressure - 1.2 atm x 101 325 Pa/atm = 121 590 Pa
V - volume - 3.94 x 10⁻³ m³
n - number of moles
R - universal gas constant - 8.314 Jmol⁻¹K⁻¹
T - temperature - 15 °C + 273 = 288 K
substituting the values in the equation
121 590 Pa x 3.94 x 10⁻³ m³ = n x 8.314 Jmol⁻¹K⁻¹ x 288 K
n = 0.200 mol
molar mass of gas is = mass / number of moles
molar mass = 12.8 g / 0.200 mol = 64 g/mol
molar mass of gas is 64 g/mol
Answer: The final temperature would be 1250.7 K.
Explanation: We are given a sample of helium gas, the initial conditions are:
(Conversion factor: 1L = 1000 mL)
(Conversion Factor: 1° C = 273 K)
The same gas is expanded at constant pressure, so the final conditions are:
To calculate the final temperature, we use Charles law, which states that the volume of the gas is directly proportional to the temperature at constant pressure.
Putting the values, in above equation, we get:
A compound differs from an element in that it can be decomposed by a chemical reaction.
A compound, by definition, is made up of two or more elements that have been combined together through a chemical bond.
Thus, the chemical bond or bonds in a compound can be decomposed by a chemical reaction giving rise to the individual elements that make up the compound.
This is unlike an element that can not be decomposed by any chemical reaction.
More on elements and compounds can be found here: brainly.com/question/5997683
