Balanced chemical equation is as;
<span> 2 Kl + Cl</span>₂ → <span>2 KCl + I</span>₂
1) Moles of I₂<span> produced;
22.4 L volume is occupied by</span> = 1 mole of I₂ at STP
So,
8.5 L of I₂ will be occupied by = X mole of I₂ at STP
Solving for X,
X = (8.5 L × 1 mol) ÷ 22.4 L
X = 0.379 Moles of I₂
2) Moles of Cl₂ used;
22.4 L I₂ utilized = 1 mole of Cl₂ gas
So,
8.5 L of I₂ will utilize = X mole of Cl₂ gas
Solving for X,
X = (8.5 L × 1 mol) ÷ 22.4 L
X = 0.379 Moles of Cl₂
3) <span>Grams of Cl</span>₂<span> used;
As,
Moles = Mass / M.mass
Or,
Mass = Moles </span>× M.mass
Mass = 0.379 mol × 70.90 g.mol⁻¹
Mass = 26.87 grams of Cl₂
Answer:
Xenon
Explanation:
Step 1: Given data
- Pressure (P): 1.00 atm (I looked it up)
Step 2: Convert the temperature to Kelvin
K = °C + 273.15 = 100.0°C + 273.15 = 373.2 K
Step 3: Calculate the number of moles (n)
We will use the ideal gas equation.
P × V = n × R × T
n = P × V / R × T
n = 1.00 atm × 0.335 L / (0.0821 atm.L/mol.K) × 373.2 K
n = 0.0109 mol
Step 4: Calculate the molar mass of the gas
M = 1.44 g / 0.0109 mol = 132 g/mol
Step 5: Identify the gas
The gas with a molar mass of about 132 g/mol is xenon.
Explanation:
The given data is as follows.
= 30.0 sec, 
= 5 min = 
= 300 sec
= 12.0 min = 
= 720 sec
Formula for adjusted retention time is as follows.
= 300 sec - 30.0 sec
= 270 sec
= 720 sec - 30 sec
= 690 sec
Formula for relative retention (
) is as follows.
= 
= 2.56
Thus, we can conclude that the relative retention is 2.56.
<span>To draw an acceptable lewis structure we must first determine the number of valance elections of the molecule in the ground state, and then adjust the molecule to refect the molecular radial cation after one or more of the electrons have been removed from its outter most shell. The lewis structure should refect the best configuation with good resonance and stability.</span>
0.53 x 200ml = 106 ml of the pH 9.0 buffer + 94 ml of the pH 10 buffer gives the desired solution
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