Answer:
C₅H₁₂.
Explanation:
- The hydrocarbon is burned in excess of oxygen to give CO₂ and H₂O.
- <em>The no. of moles of CO₂ produced = mass/molar mass </em>= 1.53 g/44.0 g/mol = <em>0.03477 mol.</em>
<em>Which is corresponding to 0.03477 mol of C.</em>
<em />
- <em>The no. of moles of H₂O produced = mass/molar mass</em> = 0.756 g/18.0 g/mol = <em>0.042 mol.</em>
<em>which corresponds to (0.042 x 2) = 0.084 moles of hydrogen.</em>
<em />
- The ratio of the number of moles of hydrogen to carbon in the composition of the compound will be 0.084 / 0.03477 = 2.4 = 12/5.
- <em>Therefore, the empirical formula of the compound under consideration is C₅H₁₂.</em>
<em></em>
Answer:
[H⁺] = 3.548 x 10⁻⁴ M.
Explanation:
∵ pH = -log[H⁺]
∴ 3.45 = -log[H⁺]
log[H⁺] = -3.45
<em>∴ [H⁺] = 3.548 x 10⁻⁴ M.</em>
The empirical formula of the compound containing 0.64 g of copper, 0.32 g of sulphur and 0.64 g of oxygen is CuSO₄
From the question given above, the following data were obtained:
Mass of Cu = 0.64 g
Mass S = 0.32 g
Mass of O = 0.64 g
<h3>Empirical formula =? </h3>
The empirical formula of the compound can be obtained as follow:
Cu = 0.64 g
S= 0.32 g
O = 0.64 g
Divide by their molar mass
Cu = 0.64 / 63.5 = 0.01
S= 0.32 / 32 = 0.01
O = 0.64 / 16 = 0.04
Divide by the smallest
Cu = 0.01 / 0.01 = 1
S= 0.01 / 0.01 = 1
O = 0.04 / 0.01 = 4
Therefore, the empirical formula of the compound is CuSO₄
Learn more: brainly.com/question/13086832
Answer: 24.1 L of 2.27 M HF will react with 3.70 kg of ![UO_2](https://tex.z-dn.net/?f=UO_2)
Explanation:
The balanced chemical reaction :
![UO_2(s)+4HF(aq)\rightarrow UF_4(s)+2H_2O(l)](https://tex.z-dn.net/?f=UO_2%28s%29%2B4HF%28aq%29%5Crightarrow%20UF_4%28s%29%2B2H_2O%28l%29)
To calculate the number of moles, we use the equation:
![\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}](https://tex.z-dn.net/?f=%5Ctext%7BNumber%20of%20moles%7D%3D%5Cfrac%7B%5Ctext%7BGiven%20mass%7D%7D%7B%5Ctext%7BMolar%20mass%7D%7D)
![\text{Number of moles of } UO_2=\frac{3.70\times 1000g}{270g/mol}=13.7moles](https://tex.z-dn.net/?f=%5Ctext%7BNumber%20of%20moles%20of%20%7D%20UO_2%3D%5Cfrac%7B3.70%5Ctimes%201000g%7D%7B270g%2Fmol%7D%3D13.7moles)
According to stoichiometry :
1 mole of
require = 4 moles of ![HF](https://tex.z-dn.net/?f=HF)
Thus 13.7 moles of
will require=
of ![HF](https://tex.z-dn.net/?f=HF)
To calculate the volume for given molarity, we use the equation:
.....(1)
Molarity of
solution = 2.27 M
Volume of
solution in L= ?
Putting values in equation 1, we get:
![54.8moles={2.27M}\times V}](https://tex.z-dn.net/?f=54.8moles%3D%7B2.27M%7D%5Ctimes%20V%7D)
![V=24.1L](https://tex.z-dn.net/?f=V%3D24.1L)
Thus 24.1 L of 2.27 M HF will react with 3.70 kg of ![UO_2](https://tex.z-dn.net/?f=UO_2)
Answer:
element having 2+ valence electrons can transfer its more than one electron that is 2 electron completely.
Explanation:
- Group IIA have 2+ valency and two electrons in its valance shell.
- Its Electropositivity is high and have the tendency to donate it two electrons.
- Element of IIA form ionic with most electronegative element.
Examples:
Cu²⁺, Mg²⁺, Sr²⁺ are examples having 2+ valance electron
one of the following is examples of element that have 2+ valence electrons
MgCl₂
Atomic number of Magnesium (Mg) is 12
Electronic Configuration of Mg:
1s², 2s², 2p⁶, 3s²
or
K =2
L = 8
M = 2
So, it have to give its 2 electrons to form a stable compound.
Similarly
Chlorine atomic number is 17
Electronic Configuration of Chlorine:
1s², 2s², 2p⁶, 3s², 3p⁵
or
K =2
L = 8
M = 7
So, it have to gain one electrons to form a stable compound and complete its octet.
So,
Two chlorine atom as a molecule gain 2 electrons from Mg²⁺ atom
So one Mg²⁺ and 2 Cl⁻ atoms form an ionic bond
where in this ionic bond Mg²⁺ transfer its 2 valence electron completely and chlorine molecule accept 2 electrons.
Cl-----Mg------Cl
So the Answer is
element having 2+ valence electrons can transfer its more than one electron that is 2 electron completely.