How many moles of O2 would be consumed if 13.673 g of V were consumed according to the reaction below?
Answers
V + O2 → VO2
From the balanced equation, you can see that 1 mole of V reacts with 1 mole of O2 to form 1 mole of VO2. This means that the mole ratio of V to O2 is 1:1.
Now, calculate the number of moles of V in 13.673 grams:
Moles of V = Mass (grams) / Molar mass (g/mol)
The molar mass of V is the atomic mass of vanadium, which is approximately 50.94 g/mol.
Moles of V = 13.673 g / 50.94 g/mol ≈ 0.2684 moles
Since the mole ratio of V to O2 is 1:1, the number of moles of O2 consumed will also be approximately 0.2684 moles.
So, 0.2684 moles of O2 would be consumed if 13.673 grams of V were consumed in the reaction.
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Answers
Answer: 61%
The reaction equation should be
CaF2 + H2SO4 → 2HF + CaSO4
For every 1 molecule CaF2 used, there will be 2 molecules of HF formed. The molecular mass of CaF2 is 78/mol while the molecular mass of HF is 20g/mol. If the yield is 100%, the amount of HF formed by 112g CaF2 would be: 112g/(78g/mol) * 2 * (20g/mol)=57.43g
The percentage yield of the reaction would be: 35g/57.43g= 60.94%
Answers
Volume = 0.30 L
M = n / V
M = 0.50 / 0.30
= 1.667 M
hope this helps!
Answers
Answer is: C) N.
Nitrogen (N) has greatest electronegativity.
Electronegativity (χ) is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.
Atoms with higher electronegativity attracts more electrons towards it, electrons are closer to that atom.
Nitrogen has electronegativity χ = 3 and other elements have less.
has the greatest attraction for electrons in a chemical bond.
Further explanation:
Electronegativity:
It is the tendency of an atom to attract the shared electrons in the bond towards itself. More the electronegativity of the atom, higher will be its tendency to attract the bonding electrons towards itself. The electronegative atom develops a partial negative charge and the electropositive atom develops a partial positive charge.
Electronegativity trends in the periodic table:
Along the period, electronegativity increases due to the increase in the nuclear charge. This results in the strong attraction of electrons.
Down the group, electronegativity decreases due to an increase in the size of elements. This results in a lesser attraction between the nucleus and the electron.
All the given elements (As, Bi, N, P) are present in the same group of the periodic table. Nitrogen is present at the top of the group so it has the highest electronegativity among the given elements. Phosphorus is present below nitrogen but above As and Bi so its electronegativity is less than nitrogen but more than the remaining elements. Arsenic is present above Bi so it has more electronegativity than Bi. Bismuth is present at the bottom of the group so it has the least electronegativity among the given elements.
Therefore, nitrogen has the greatest tendency to attract electrons towards itself in a chemical bond.
Learn more:
1. Which ion was formed by providing the second ionization energy? brainly.com/question/1398705
2. Write a chemical equation representing the first ionization energy for lithium: brainly.com/question/5880605
Answer details:
Grade: High School
Subject: Chemistry
Chapter: Periodic classification of elements
Keywords: electronegativity, electron, N, P, As, Bi, group, period, increase, decrease, attraction, chemical bond, nitrogen, phosphorus, arsenic, bismuth.
Answers
Basically, a solution is just any of the same mixture, which is solid-solid, liquid-liquid, and gas-gas.
metal and nonmetal
metalloid and nonmetal
two metals
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Answer: The correct answer is metal and non-metal.
Explanation:
Elements are mainly divided into 3 classes in the periodic table.
1.) Metals: The element which lie on the left side of the periodic table are mainly metals. These elements loose electron easily and form positively charged species. These elements are present in the highest proportion in the periodic table.
2.) Non-metals: The elements which lie on the right side of the periodic table are considered as non-metals. These elements gain electrons easily and form negatively charged species.
3.) Metalloids: These lie between metals and non-metals and show the properties of both metals and non-metals.
Copper lie in the period 4 and group 11 of the periodic table and it can easily loose electron and hence, it is considered as a metal.
Chlorine lie in the period 3 and group 17 of the periodic table and it can easily gain electron and hence, considered as a non-metal.
Therefore, the correct answer is metal and non-metal.
b. atoms or molecules.
c. elements or compounds.
d. mixtures or substances.
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Answer:C
Explanation:cause I just took the test and I can confirm