Answer: 0.209 M
Explanation:
Moles of = 2.00 mole
Moles of = 1.50 mole
Volume of container = 5.00 L
Initial concentration of =
Initial concentration of =
The given balanced equilibrium reaction is,
Initial conc. 0.400 M 0.300M 0 M 0 M
At eqm. conc. (0.400-x) M (0.300-x) M (x) M (x) M
The expression for equilibrium constant for this reaction will be,
Now put all the given values in this expression, we get :
By solving the term 'x', we get :
x = 0.209 M
Concentration of at equilibrium = x M = 0.209 M
<span>by performing more experiments</span>
Answer: The number of moles in 250.0 L of He at STP is 11.0 mole.
Explanation:
- It is known that 1.0 mole of a gas at STP conditions will occupy 22.7 L.
- To show this information: STP means that T = 0.0 °C = 273.15 K and P = 1.0 kPa = (100/101.325) = 0.9869 atm.
- From the ideal gas law: PV = nRT.
- Where, P is the pressure in atm <em>(P = 1.0 atm at STP).</em>
- n is the number of moles (n = 1.0 mole).
- R is the general gas constant (R = 0.0821 L.atm/mol.K).
- T is the temperature in K (T = 273.15 K at STP).
- and now we can get the volume of 1.0 mole at STP: V = nRT/P
- V = (1.0 mole x 0.0821 L.atm/mol.K x 273.15 K) / (0.9869 atm) = 22.7 L.
- Now, we can get the number of moles of 250.0 L of He at STP:
<em>Using cross multiplication:</em>
1.0 mole → 22.7 L
??? mole → 250.0 L
- The number of moles in 250.0 L of He at STP = (250.0 L x 1.0 mole) / (22.7 L) = 11.01 mole ≅ 11.0 mole.
Answer:
See Explanation
Explanation:
It is a common observation that a strip of aluminium metal in aqueous copper(II)Sulfate does not show any visible reaction. Aluminium is normally expected to displace copper in solution since it is higher than copper in the electrochemical series.
The reason for this is that aluminium forms an oxide film around its surface which prevents reaction with aqueous copper(II)Sulfate. This oxides film protects the aluminium surface such that it is now unable to react with the aqueous copper(II)Sulfate