Answer:
The correct answer is 5.0 L
Explanation:
STP are defined as T=273 K and P= 1 atm
By using the ideal gas equation, we can calculate the number of moles (n) of the gas at a volume V=2.5 L:
PV= nRT
⇒n= (PV)/(RT) =(1 atm x 2,5 L)/(0.082 L.atm/K.mol x 273 K)= 0.112 mol
For a sample of argon gas, with the same number of moles (0.112 mol) but twice the temperature (T = 273 K x 2= 546 K):
V= (nRT)/P = (0.112 mol x 0.082 L.atm/K.mol x 546 K)/1 atm = 5.0 L
That is consistent with the fact that when a gas is heated, it expanses. So, if the temperature increases twice, the volume also increases twice.
Answer:
single displacement reaction
I believe propane burns to form water vapor and carbon dioxide
Answer:
1.208x10⁻³M and 392.5ppm La(NO3)3
Explanation:
The reaction that occurs is:
La2O3 + 6HNO3 → 2La(NO3)3 + 3H2O
Molarity is defined as the moles of solute (In this case, LaO3) per liter of solution. And ppm, are mg of solute per liter of solution.
To solve this question we must find the moles of La(NO3)3 produced and its mass in milligrams to find molarity and ppm:
<em>Moles La2O3 -Molar mass: 325.81g/mol-</em>
0.1968g * (1mol / 325.81g) = 6.04x10⁻⁴ moles La2O3
<em>Moles La(NO3)3:</em>
6.04x10⁻⁴ moles La2O3 * (2mol La(NO3)3 / 1mol La2O3) = 1.208x10⁻³ moles La(NO3)3
<em>Molarity:</em>
1.208x10⁻³ moles La(NO3)3 / 1L =
<h3>1.208x10⁻³M</h3>
<em>Mass La(NO3)3 -Molar mass: 324.92g/mol-</em>
1.208x10⁻³ moles La(NO3)3 * (324.92g / mol) = 0.392.5g La(NO3)3
In mg:
392.5mg La(NO3)3 / 1L =
392.5ppm La(NO3)3
