I suspect that the pressure of this change is constant therefore
The equation is used from the combined gas law. (When pressure is constant both P's will cancel out P/P = 1)
V/T = V/T
Initial Change
Initially we have 2L at 20 degress what temperature will be at 1L.
2/20 = 1/T
0.1 = 1/T
0.1T = 1
T = 1/0.1
T = 10 degress celsius.
Hope this helps if you won't be able to understand what is the combined gas law just tell me :).
x = = 0.50 M
Answer:
In order to produce some SbCl5, a 1.00 mole sample of SbCl3 is first placed in an empty 2.00 liter container maintained at a temperature different from 182oC. At this temperature, Kc, equals 0.117. How many moles of Cl2 must be added to this container to reduce the number of moles of SbCl3 to 0.700 mole at equilibrium
Moles Cl2 that must be added = 0.40 mol
Explanation:
K = ( = 0.117
Equilibrium concentrations:
= (1.00 - 0.70) mol / 2.00 L = 0.15 M <<---why is it 1.00-0.70???
= 0.700 mole / 2.00L = 0.350 M
= x
Kc = ÷ (0.15) = 0.117
Moles Cl2 at equilibrium = 0.050 mol L x 2.00 L = 0.10 mol
Moles Cl2 needed to make 0.300 mol SbCl3 into SbCl5 = 0.30 mol
Moles Cl2 that must be added = 0.40 mol
Answer:
0.0198 M
Explanation:
Given data
- Mass of CaCl₂ (solute): 5.51 g
- Volume of solution: 2.50 L
Step 1: Calculate the moles of solute
The <em>molar mass of CaCl₂</em> is 110.98 g/mol. The moles corresponding to 5.51 g are:
5.51 g × (1 mol/110.98 g) = 0.0496 mol
Step 2: Calculate the molarity of the solution
<em>M = moles of solute / liters of solution</em>
M = 0.0496 mol / 2.50 L
M = 0.0198 M
Answer: The answer is true.
Explanation: Avogadro's number is a mole, which concludes that this statement is true.