m(O2)=50g
m(H2)=50g
m(H2O)-?
n2(H2)-?
2H2 + O2 = 2H2O
n(O2)= m (O2)/M(O2) =50g / 32 g/mol= 1,56 mol.
n(H2)= m (H2)/M(H2) =50g / 2 g/mol= 25 mol.
Since oxygen gas is the limiting reactant,
n(O2)< 2 n(H2) from reaction.
n(H2O)= 2n(O2)= 2n (H2 reac.)=2*1,56 mol=3,12mol.
m(H2O)=n(H2O)*M(H2O)= 3,12mol* 18 g/mol.
n2(H2)= n(H2) - n (H2 reac.)=25mol - 3,12mol=21,88mol.
Its A) Shared equally
Non-polar bonds are a type of chemical bond where two atoms share a pair of electrons with each other.
Answer : Option C) wrapped in camouflage colored cloth.
Explanation : If you want a safe and best way to get out of the woods after having harvested a wild turkey to avoid getting spotted by other hunter is to cover the turkey with camouflage colored cloth.
Answer:
Explanation:
CH₃CHOHCOOH ⇄ CH₃CHOHCOO⁻ + H⁺
ionisation constant = 1.36 x 10⁻⁴ .
molecular weight of lactic acid = 90 g
moles of acid used = 20 / 90
= .2222
it is dissolved in one litre so molar concentration of lactic acid formed
C = .2222M
Let n be the fraction of moles ionised
CH₃CHOHCOOH ⇄ CH₃CHOHCOO⁻ + H⁺
C - nC nC nC
By definition of ionisation constant Ka
Ka = nC x nC / C - nC
= n²C ( neglecting n in the denominator )
n² x .2222 = 1.36 x 10⁻⁴
n = 2.47 x 10⁻²
nC = 2.47 x 10⁻² x .2222
= 5.5 x 10⁻³
So concentration of hydrogen or hydronium ion = 5.5 x 10⁻³ g ion per litre .
Explanation:
The given data is as follows.
Moles of oxygen gas = 0.150 mol, Moles of nitrogen gas = 0.116 mol
Moles of argon gas = 0.211 mol, Volume of the flask = 0.5 L
Temperature = 298 K
So, total number of moles will be calculated as follows.
= (0.150 + 0.116 + 0.211) mol
= 0.477 mol
Now, using ideal gas equation we will calculate the total pressure of given gas mixture as follows.
PV = nRT
P = 23.34 atm
Mole fraction of gas will be calculated as follows.
Mole fraction =
=
= 0.243
Using Dalton's law,
where, = partial pressure of a gas
= total pressure
= mole fraction of gas
Therefore, putting the values into Dalton's law to calculate the partial pressure of nitrogen gas as follows.
=
= 5.67 atm
Thus, we can conclude that the partial pressure of into the given mixture is 5.67 atm.