Based on the data provided;
- number of moles of helium gas is 1.25 moles
- pressure at peak temperature is 259.3 kPa
- internal pressure is above 256 kPa, therefore, the balloon will burst.
- pressure should be reduced to a value less than 256 kPa by reducing the temperature
<h3>What is the ideal has equation?</h3>
The ideal gas equation relatesthe pressure, volume, moles and temperature of a gas.
The moles of helium gas is calculated using the Ideal gas equation:
n is the number of moles of gas
R is molar gas constant = 8.314 L⋅kPa/Kmol
P is pressure = 239 kPa
T is temperature = 21°C = 294 K
V is volume = 12.8 L
Therefore;
n = PV/RT
n = 239 × 12.8 / 8.314 × 294
n = 1.25 moles
The number of moles of helium gas is 1.25 moles
At peak temperature, T = 46°C = 319 K
Using P1/T1 = P2/T2
P2 = P1T2/T1
P2 = 239 × 319/294
P2 = 259.3 kPa
The pressure at peak temperature is 259.3 kPa
At 42°C, T = 315 K
Using P1/T1 = P2/T2
P2 = P1T2/T1
P2 = 239 × 315/294
P2 = 256.07 kPa
Since the internal pressure is above 256 kPa, the balloon will burst.
The pressure should be reduced to a value less than 256 kPa by reducing the temperature.
Learn more about gas ideal gas equation at: brainly.com/question/12873752
Answer:
b. gelatin
Explanation:
a homogeneous noncrystalline consisting of large molecules or ultramicroscopic particles of one substance.
Answer:
7.3 mole
Explanation:
1 C6H10S gives 10H
0.73 mole of C6H10S gives X mole of Hydrogen
X= 0.73×10=7.3mole
Answer: 1.79 x 10^-5
Explanation: The equilibrium constant of a reaction can be calculated from the quotient of the concentrations of the products over the concentrations of the reactants, with each termed raised to their respective stoichometric coefficients.
For acetic acid, this equilibrium expression is:
![Kc=\frac{[H+] [CH3COO-]}{[CH3COOH]}](https://tex.z-dn.net/?f=Kc%3D%5Cfrac%7B%5BH%2B%5D%20%5BCH3COO-%5D%7D%7B%5BCH3COOH%5D%7D)
Replacing the equilibrium concentrations given by the exercise into the expression above, the equilibrium constant, Kc will be obtained and it is found to be equal to 1.79 x 10^-5.
Answer:
55.85 grams of Fe is formed.
Explanation:
Identify the reaction:
2Fe₂O₃ + 3C → 4Fe + 3CO₂
Identify the limiting reactant, previously determine the mol of each reactant
(mass / molar mass)
10 g / 12 g/m = 0.83 moles C
80 g / 159.7 g /m = 0.500 moles Fe₂O₃
2 moles of oxide need 3 moles of C, to react
0.5 moles of oxide, will need ( 0.5 . 3)/ 2 = 0.751 mol
I have 0.83 moles of C, so C is the excess.
The limiting is the oxide.
3 mol of C need 2 mol of oxide to react
0.83 mol of C, will need (0.83 . 2)/ 3 = 0.553 mol of oxide, and I only have 0.5 (That's why Fe₂O₃ is the limiting)
Ratio is 2:4 (double)
If I have 0.5 moles of oxide, I will produce the double, in the reaction.
1 mol of Fe, will be produce so its mass is 55.85 g
