T<span>he balanced reaction is as follows;
Ca(OH)</span>₂<span> + 2HCl ---> CaCl</span>₂<span> + 2H</span>₂<span>O
stoichiometry of Ca(OH)</span>₂<span> to HCl is 1:2
number of moles of Ca(OH)</span>₂<span> reacted = 0.120 mol/L x 0.0240 L = 0.00288 mol according to molar ratio of 1:2 number of HCl moles reacted = twice the number of Ca(OH)</span>₂<span> moles reacted
number of HCl moles reacted = 0.00288 mol x 2 = 0.00576 mol
number of HCl moles in 160 mL - 0.00576 mol
therefore number of HCl moles in 1000 mL - 0.00576 mol / 160 mL x 1000 mL = 0.036 mol
molarity of HCl = 0.036 M</span>
Hello!
For this problem, we will be applying <em>Charles' Law</em>:
V1/T1 = V2/T2
Now that we have the formula, let's convert the temperature to Kelvin.
27 + 273 = 300K
Let's plug everything in now!
10/300 = 12.0/x
Simplified:
1/30 = 12.0/x
Cross-multiply:
1x = 30*12.0
<u>x = 360</u>
<em>Check!</em>
10/300 = 12/360
300*12 = 360*10
3600 = 3600
Therefore, you would have to heat the gas at a temperature of 360K in order to raise the volume to 12.0L.
Balanced chemical reaction: 2K(s) + 2H₂O(l) → 2KOH(aq) + H₂(g).
KOH is inorganic compound p<span>otassium hydroxide, a strong base.
H</span>₂ is hydrogen gas.
In balanced chemical reaction number of atoms on both side of chemical reaction must be same. There are two potassium atoms, four hydrogen atoms and two oxygen atoms on both side of reaction.
Answer:
You will have 19.9L of Cl2
Explanation:
We can solve this question using:
PV = nRT; V = nRT/P
<em>Where V is the volume of the gas</em>
<em>n the moles of Cl2</em>
<em>R is gas constant = 0.082atmL/molK</em>
<em>T is 273.15K assuming STP conditions</em>
<em>P is 1atm at STP</em>
The moles of 63g of Cl2 gas are -molar mass: 70.906g/mol:
63g * (1mol / 70.906g) = 0.8885 moles
Replacing:
V = 0.8885mol*0.082atmL/molK*273.15K/1atm
V = You will have 19.9L of Cl2
