The final temperature = -145.24K or 127°C.
According to the data given,
T1= 88°C = 361.15K
V1= 9.6 L
V2= 3.4 L
T2= ?
We know that, according to Charles's law,
T1/V1=T2/V2
T2= T1*V2/V1
T2= 127°C or -145.24K
The final temperature = -145.24K or 127°C
<h3>What does Charles law state?</h3>
According to Charles' law, when the pressure is held constant, the volume of a given amount of gas is precisely proportional to its temperature on the kelvin scale.
<h3>What connection exists between volume and temperature?</h3>
- In layman's words, the volume of a fixed mass of gas is exactly proportional to temperature at constant pressure.
- When a constant mass of gas is cooled, its volume decreases, and when the temperature is elevated, its volume grows.
<h3>What are the applications of Charles law?</h3>
- A hot air balloon drifting through the air is an illustration of Charles Law in action.
- The air within the balloon is heated by a torch, which causes the air molecules to move more quickly and disperse.
- This causes the air inside the balloon to be less dense than the air outside, which causes the balloon to float.
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We use the given masses of the reactants to calculate the moles of Mn and Cl. Empirical formula represents the simplest mole ratio of atoms present in a compound.
Moles of Mn = 
Moles of Cl = 
= 0.710 mol Cl
Simplest mole ratio: 
So the empirical formula is 
Answer:
Explanation:
The equation that relates standard Gibbs free energy, ΔG, with equilibrium constant, K, is:
ΔG = -RT ln K
<em>Where R is gas constant, 8.314J/molK, and T is absolute temperatue (30.0°C + 273.15 = 303.15K).</em>
<em />
Replacing (110kJ = 110000J):
110000J/mol = -8.314J/molK*303.15K ln K
-43.644 = lnK
1.11x10⁻¹⁹ = K
<em />
<u>We are given:</u>
Mass of water: 119 grams
We know that one mole of a gas occupies 22.4L of volume
<u>Number of moles of water:</u>
Number of moles = given mass / Molar mass
Number of moles = 119 / 18 [molar mass of water = 18 grams/mol]
Number of moles = 6.61 moles
<u>Volume occupied:</u>
Volume = number of moles * 22.4 L
Volume = 6.61 * 22.4
Volume = 148L
Volume (in mL) = 1.48 * 10⁻¹ mL
. For He, The outermost electrons are 2.
( where, n = 2, 3, 4, 5, 6 and 7 respectively). For all the other gases, the outermost electrons are 8.