State one conclusion from Rutherford experiment that contradicted one conclusion made by Thompson
Answers
Answer:
One conclusion from Rutherford's experiment that greatly contradicted Thompson's experiment is that 'atoms are mostly empty space, with positively charged nucleus'.
Explanation:
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Answers
the balanced chemical equation for decomposition of HgO is as follows
2HgO --> 2Hg + O₂
stoichiometry of HgO to O₂ is 2:1
number of HgO moles heated are - 3.00 g / 216.59 g/mol = 0.0139 mol
according to stoichiometry of reaction -
number of O₂ moles formed = 0.0139 mol/ 2 = 0.00695 mol
mass of O₂ to be formed - 0.00695 mol x 32.00 g/mol = 0.2224 g
but the actual yield = 0.195 g
percent yield = actual yield / theoretical yield x 100 %
percent yield = 0.195 g / 0.2224 g x 100 % = 87.7 %
answer is 87.7 %
Answer:
The correct answer is 87.8%
Answers
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
Considering the definition of molar mass and molarity, the volume of each compound is:
- NaCl= 0.1355 L
- C₂H₆O = 0.0622 L
- CH₃COOH = 0.047 L
Definition of molar mass
The molar mass of substance is a property defined as its mass per unit quantity of substance, in other words, molar mass is the amount of mass that a substance contains in one mole.
Definition of molarity
Molar concentration or molarity is a measure of the concentration of a solute in a solution and indicates the number of moles of solute that are dissolved in a given volume.
The molarity of a solution is calculated by dividing the moles of solute by the volume of the solution:
Molarity is expressed in units.
Volume required
You know that the molar mass of each compound is:
- NaCl = 58.44 g/mol
- C₂H₆O = 46.06 g/mol
- CH₃COOH = 60.0 g/mol
On the other side, you know that the mass of each compound is:
- NaCl = 2.14 g
- C₂H₆O = 4.30 g
- CH₃COOH = 0.85 g
Then, considering the definition of molar mass, the amount of moles of each compound is:
- NaCl =
= 0.0366 moles
- C₂H₆O =
= 0.0933 moles
- CH₃COOH =
= 0.0141 moles
The molarity of each compound is:
- NaCl = 0.27 M
- C₂H₆O = 1.50 M
- CH₃COOH = 0.30 M
Considering the molarity, the volume of each compound is calculated as:
- NaCl =
= 0.1355 L
- C₂H₆O =
= 0.0622 L
- CH₃COOH =
= 0.047 L
Learn more about
molar mass:
molarity:
number of moles : 2.14 / 58.44 = 0.0366 moles
V = n / M => 0.0366 / 0.270 = 0.1355 L
__________________________________________
b) C2H6O = 46.06 g/mol
number of moles : 4.30 / 46.06 = 0.0933 moles
V = n / M => 0.0933 / 1.50 = 0.0622 L
___________________________________________
c) CH3COOH = 60.0 g/mol
number of moles : 0.85 / 60.0= 0.0141 moles
V = n / M => 0.0141 / 0.30 = 0.047 L
___________________________________________
hope this helps!
Answers
IF there is a decrease in the temperature at the equator then it is possible that there is an increase in the speed of current.
All matter is composed of very small particles called atoms.
All atoms of a given element are identical.
Atoms cannot be created, destroyed, or subdivided.
Atoms combine with or separate from other atoms.
Atoms combine with each other.
Answers
1) all elements are made up of atoms.
2) atoms are so small that they cannot be divided any further.
3) an atom can neither be destroyed nor be formed.
4) atoms of an element are similar, they posses same mass and same properties.
5) atoms of different elements combine in a definite ratio to form compounds.
Due to further experimentation it was concluded that atom is made up of small particles identified as proton, neutrons, and electrons. They can be further subdivided.
Another change is the presence of isotopes of atoms of different elements. Hence, atoms of the same element can also have different masses.