Answer:
The balanced chemical equation for the reaction is:
2 C2H6 + 7 O2 → 4 CO2 + 6 H2O
From the equation, 2 moles of ethane react with 7 moles of oxygen gas to produce 6 moles of water.
First, we need to determine which reactant is limiting. To do this, we can use the given masses and convert them to moles using the molar masses of the compounds:
n(C2H6) = 3.01 g / 30.07 g/mol = 0.100 mol
n(O2) = 19.3 g / 32.00 g/mol = 0.603 mol
The mole ratio of C2H6 : O2 is 2 : 7, so to react completely with 0.100 mol of C2H6, we need:
n(O2) = (7/2) x 0.100 mol = 0.350 mol
Since we have more than 0.350 mol of O2, O2 is not the limiting reactant. Therefore, the limiting reactant is C2H6.
The theoretical yield of H2O can be calculated from the number of moles of C2H6:
n(H2O) = (6/2) x 0.100 mol = 0.300 mol
Finally, we can convert the number of moles of H2O to grams:
m(H2O) = n(H2O) x M(H2O)
m(H2O) = 0.300 mol x 18.02 g/mol
m(H2O) = 5.41 g
Therefore, the theoretical yield of H2O formed is 5.41 g. Rounded to three significant figures, the answer is 5.41 g.
Explanation:
- Preparation of NaPO4 solution (So): A solution (So) of sodium phosphate is to be prepared of molar concentration 0.1 mol/L. mL. 100 Given M(Na3PO)=164 g/mol. and a volume 1.1- Calculate the mass of sodium phosphate needed to prepare this solution. Deduce its mass concentration (Cm). 1.2 - Write the materials and glassware needed. 1.3- Write the equation of dissolution of sodium phosphate. 1.4- Determine the molar concentration of Na ions in this solution
Answer:
Explanation:
1.1 we have to find mass of Na3PO4;
for that we have to Calculate the moles of Na3PO4 needed:
volume is 100mL = 0.1L
Molar concentration = Moles of solute / Volume of solution in L
0.1 mol/L = Moles of Na3PO4 / 0.1 L
Moles of Na3PO4 = 0.1 mol/L * 0.1 L
Moles of Na3PO4 = 0.01 mol
Now, Calculate the mass of Na3PO4 needed:
so, Mass = Moles of Na3PO4 * Molar mass of Na3PO4
Mass = 0.01 mol * 164 g/mol
Mass = 1.64 g of Na3PO4.
1.2 materials and glassware needed:
1.64 g Sodium phosphate (Na3PO4)
100 mL volumetric flask
weighing balance
Distilled water
Glass rod
Pipette and burette
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A potassium ion can combine with several monatomic and polyatomic ions to form compounds.
An example of a potassium compound containing both ionic and covalent bonds is , and an example containing only ionic bonds is .
An example of a potassium compound containing both ionic and covalent bonds is potassium chloride and an example containing only ionic bonds is potassium sulfite.
A potassium ion (K+) can combine with various monatomic and polyatomic ions to create compounds through different types of chemical bonds. In the context of potassium compounds, both ionic and covalent bonds can be observed.
An example of a potassium compound that exhibits both ionic and covalent bonds is potassium chloride (KCl). In this compound, potassium donates its valence electron to chlorine, forming an ionic bond between the positively charged potassium ion and the negatively charged chloride ion. However, there is also some degree of covalent character present in the compound, as the electron is not fully transferred from potassium to chlorine. This partial sharing of electrons results in a degree of covalent bonding.
On the other hand, an example of a potassium compound containing only ionic bonds is potassium sulfate (K2SO4). In this compound, two potassium ions (K+) combine with one sulfate ion (SO4^2-) through ionic bonds. The transfer of electrons is complete, resulting in a strong electrostatic attraction between the oppositely charged ions, forming an entirely ionic compound.
In summary, potassium chloride exemplifies a potassium compound containing both ionic and covalent bonds, whereas potassium sulfate represents a potassium compound consisting solely of ionic bonds.
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A potassium ion can combine with several monatomic and polyatomic ions to form compounds.
An example of a potassium compound containing both ionic and covalent bonds is ___(potassium chloride, potassium hydride, potassium nitrate, potassium oxide), and an example containing only ionic bonds is _____(potassium chloride, potassium hypochlorite, potassium sulfate, potassium sulfite).
how much energy is required to vaporize 2 kg of copper
It would require approximately 600 kilojoules of energy to vaporize 2 kg of copper.
To calculate the energy required to vaporize a substance, we need to consider the heat of vaporization, which is the amount of energy required to convert a given amount of substance from its liquid state to its gaseous state at a constant temperature.
The heat of vaporization for copper is approximately 300 kJ/kg (kilojoules per kilogram) at its boiling point, which is around 2567 degrees Celsius (4649 degrees Fahrenheit). This means that for every kilogram of copper, 300 kJ of energy is needed to vaporize it.
Given that you have 2 kg of copper, we can calculate the total energy required as follows:
Energy = Heat of Vaporization × Mass
Energy = 300 kJ/kg × 2 kg
Energy = 600 kJ
Therefore, it would require approximately 600 kilojoules of energy to vaporize 2 kg of copper.
It's worth noting that the heat of vaporization can vary slightly depending on the purity of the copper and the specific conditions, such as temperature and pressure. The value provided here is an approximation. Additionally, it's important to handle copper and any high-temperature processes with caution, as they can pose safety hazards.
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Calculate the ratio of the moles of produced to the moles of each of the reactants used. (Write two separate ratios.)
Ratio of moles of NH₃ produced to moles of N₂ used: 2 moles of NH₃ / 1 mole of N₂
Ratio of moles of NH₃ produced to moles of H₂ used: 2 moles of NH₃ / 3 moles of H₂
What is the mole ratio of the reaction?From the balanced chemical equation:
N₂ + 3 H₂ ⟶ 2 NH₃
We can determine the ratio of moles of products to the moles of each reactant.
Ratio of moles of NH₃ produced to moles of N₂ used:
From the balanced equation, we can see that 1 mole of N₂ reacts to produce 2 moles of NH₃. Therefore, the ratio is:
2 moles of NH₃ / 1 mole of N₂
Ratio of moles of NH₃ produced to moles of H₂ used:
From the balanced equation, we can see that 3 moles of H₂ react to produce 2 moles of NH₃. Therefore, the ratio is:
2 moles of NH₃ / 3 moles of H₂
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Given the equation of reaction;
N₂ + 3 H₂ ---> 2 NH₃
Calculate the ratio of the moles of produced to the moles of each of the reactants used. (Write two separate ratios.)
Which structure is the Lewis structure for ammonia (NH3)?
A.
A bond line structure of a compound has N H H H. The nitrogen has two dots at its bottom represents a lone pair of electrons.
B.
A bond line structure of a compound has H N H in the linear plane and hydrogen is branching upward, and the compound is H N (H) H.
C.
A bond line structure of a compound has H N H in linear plane and a hydrogen is branching upward, and the compound is H N (H) H. The nitrogen has two dots at its bottom represents a lone pair of electrons.
D.
A bond line structure of a compound has H N H H. The nitrogen has two dots on its top represents a lone pair of electrons.
Answer: **
H-N-H
|
H
Explanation:
Look at a periodic table to determine how many electrons you need to account for. Hydrogen (H) only has 1 electron, while Nitrogen (N) has 5. We have three Hydrogen atoms and one Nitrogen atom, so the total number of electrons will be 3 * 1 + 5 = 8 e-.
Now, place the center atom, which will be Nitrogen and place the three Hydrogens on three sides of it as above in the answer. You should use single bonds for this. Each single bond is a pair of electrons, so since we have three single bonds so far, we have accounted for 2 * 3 = 6 electrons. However, we need 2 more electrons for the total of 8. We put these electrons in as a lone pair above Nitrogen.
We check to see if everything follows the octet rule: Nitrogen has three single bonds, so that's 6 e-, as well as one lone pair, so that's another 2 e- for a total of 8 e-. Check. Now look at Hydrogen: H is the only element whose full orbital is 2 e-. Each H has a single bond with Nitrogen, so each does have 2 e-.
Thus, we know this is the correct diagram, and we are done.
Explanation:
A bond line structure of a compound has H N H in linear plane and a hydrogen is branching upward, and the compound is H N (H) H. The nitrogen has two dots at its bottom represents a lone pair of electrons. So ,the correct answer is option C.
The correct Lewis structure for ammonia ([tex]NH_3[/tex]) is option C. It shows a bond line structure with three hydrogen atoms (H) bonded to a central nitrogen atom (N) in a linear plane.
One hydrogen atom branches upward from the plane. Additionally, the nitrogen atom in this structure has two dots at its bottom, indicating a lone pair of electrons. This arrangement follows the octet rule, as nitrogen has formed three covalent bonds with hydrogen, completing its valence shell. The lone pair on nitrogen gives ammonia its characteristic properties.
Thus, option C accurately represents the Lewis structure of ammonia, showing the bonding and lone pair arrangement of its atoms.
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