In order to solve this question, you use the formula C1V1=C2V2; C1 and V1 represent the concentration and volume of the starting solution respectively, and C2 and V2 represent the concentration and volume of the final solution respectively.
In this case, C1 is 10.5, V1 is unknown, C2 is 0.98 and V2 is 3 liters.
(10.5)(x)=(0.98)(3) (divide both sides by 10.5)
X=0.28 L
This means that you will use 0.28 L of the 10.5 M solution and 2.27 L (3 L-0.28 L) of water to make 3 L of a 0.98 M solution.
Hope this helps
The expansion work on an irreversible system is equal to:
W = - PV
Assuming that the gas is ideal, therefore:
PV = nRT
[P=pressure, V=volume, n=number of moles, R=gas constant,
T=absolute temperature]
Therefore,
W = -nRT
W = -(1 mol) * (8.314 J / mol K) * (1250 K)
W = -10,392.50 J
Therefore about 10,392.50 J or 10.4 kJ of work is done on
the system.
To solve for the absolute temperature, we assume ideal gas
behaviour so that we use the equation:
PV = nRT
or T = PV / nR
So calculating:
T = [6.6 atm * 0.40 L] / [(2.4g / 28g/mol) * 0.08205746 L
atm / mol K]
<span>T = 375.35 K</span>
Answer:
22 in total but round it up to 23
Because that's the only way they can
