Fluorine in compounds is always assigned an oxidation number of -1
135.1kPa
Explanation:
Given parameters:
T1 = 27°C
P1 = 101.325 kPa
T2 = 127°C
Unknown:
P2 = ?
Solution:
Using a derivative of the combined gas law where we assume that the gas has a constant volume, we can solve for the unknown.
At constant volume:
P1 is the initial pressure
T1 is the initial temperature
P2 is the final pressure
T2 is the final temperature
Take the given temperature to K
T1 = 27 + 273 = 300K
T2 = 127 + 273 = 400K
Input the variables:
P2 = 135.1kPa
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Answer:
the mole fraction of Gas B is xB= 0.612 (61.2%)
Explanation:
Assuming ideal gas behaviour of A and B, then
pA*V=nA*R*T
pB*V=nB*R*T
where
V= volume = 10 L
T= temperature= 25°C= 298 K
pA and pB= partial pressures of A and B respectively = 5 atm and 7.89 atm
R= ideal gas constant = 0.082 atm*L/(mol*K)
therefore
nA= (pA*V)/(R*T) = 5 atm* 10 L /(0.082 atm*L/(mol*K) * 298 K) = 2.04 mole
nB= (pB*V)/(R*T) = 7.89 atm* 10 L /(0.082 atm*L/(mol*K) * 298 K) = 3.22 mole
therefore the total number of moles is
n = nA +nB= 2.04 mole + 3.22 mole = 5.26 mole
the mole fraction of Gas B is then
xB= nB/n= 3.22 mole/5.26 mole = 0.612
xB= 0.612
Note
another way to obtain it is through Dalton's law
P=pB*xB , P = pA+pB → xB = pB/(pA+pB) = 7.69 atm/( 5 atm + 7.89 atm) = 0.612
According to Balance chemical equation,
N₂ + 3 H₂ → 2 NH₃
1 mole of Nitrogen reacts with 3 moles of Hydrogen to produce 2 mole of Ammonia.
It is known that i mole of any gas at standard temperature and pressure occupies 22.4 L of Volume. So, we can also say,
22.4 L (1 × 22.4) of Nitrogen gas (in question it is taken in excess) reacts with 67.2 L (22.4 × 3) of Hydrogen gas to produce 44.8 L (22.4 × 2) of Ammonia.
Result:
44.8 L is the correct answer.
B. Shrimp burrow.
Explanation:
A trace fossil is a fossil left by the animal, such as a foot print or a burrow. It is not part of the actual animal.
