A 1170.-gram sample of NaCl() completely reacts, producing 460. grams of Na(). What is the total mass of Cl2(g) produced?
Answers
2 mol * 23 g Na = 46 g
2*35,5 g Cl = 71
46 g Na --------- 71 g Cl₂
460 g Na -------- ?
mass ( Cl₂) = 460 . 71 / 46
Mass (Cl₂) = 32660 / 46
m= 710 g of Cl₂
hope thips helps
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Based on the Periodic Table, explain why Na and Khave similar chemical properties
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Answers
Answer : The concentration of solution is, 0.45 M
Solution :
The given balanced reaction is,
The moles ratio of and
is, 1 : 1 that means 1 mole of HCl neutralizes by the 1 mole of ammonia.
According to the neutralization law,
where,
= molarity or concentration of
solution = ?
= volume of
solution = 25 ml
= molarity of concentration HCl solution = 0.25 M
= volume of HCl solution = 45 ml
Now put all the given values in the above law, we get the concentration of solution.
Therefore, the concentration of solution is, 0.45 M
no. of mol of hcl = vol. (L) x molarity = 0.045 × 0.25 = 0.01125mol
ratio of hcl:nh3 after balancing eqn = 1:1
no. of mol of nh3 that is completely neutralised by hcl = 0.01125 × 1 = 0.01125mol
therefore, concentration of nh3 = mol / total volume (L) = 0.01125mol / 0.025L= 0.45M
Answers
B. isotopes
C. elements
D. molecules
Answers
Ions have negative charges. They also contain more protons than electrons.
I hope this helps!
Answer:
IONS
Explanation:
Answers
Answer: There are 6 mole of oxygen present in 1 mole of .
Explanation:
The given formula of compound is . In this compound, there are 1 mole of magnesium, 2 mole of chlorine and
mole of oxygen atom.
Therefore, we can conclude that the total number of moles of oxygen atoms present in 1 mole of is 6 mole.
Thats the question right? the answer is 6
O
2
COX
2
will be produced from
97.0
g
97.0 g97, point, 0, start text, space, g, end text of
C
3
H
8
CX
3
HX
8
, assuming
O
2
OX
2
is available in excess?
Answers
Final answer:
Given 97.0 g of propane (C3H8), about 6.6 moles of CO2 will be produced according to the balanced chemical equation for the combustion of propane.
Explanation:
The question asks how many moles of CO2 will be produced from 97.0 g of C3H8, assuming O2 is available in excess.
The balanced chemical equation for the combustion of propane (C3H8) is C3H8 + 5O2 → 3CO2 + 4H2O. This tells us that one mole of propane produces three moles of CO2.
First, we need to find the moles of propane. The molar mass of propane is approximately 44.09 g/mole. So, 97.0 g of propane corresponds to approximately 2.2 moles. Therefore, 2.2 moles of propane produce 2.2 * 3 = 6.6 moles of CO2.
Learn more about moles of CO2 produced here:
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Answers
Answer:
K < Fe < Br < Kr
Explanation:
Given chemical elements;
Potassium
Iron
Bromine
Krypton
Problem; arrange in order of increasing electronegativity
Solution:
The electronegativity of an element measures the relative tendency with which the atoms of the element attracts valence electrons in the chemical bond.
To solve this problem, we are going to use values of electronegativity from the Pauling's electronegativity table of elements;
For;
Potassium = 0.8
Iron = 1.83
Bromine = 2.8
Krypton = 3.0
So;
K < Fe < Br < Kr