Answer:
<h2> 162g/mol</h2>
Explanation:
The question is incomplete. The complete question includes the information to find the empirical formula of nicotine:
<em>Nicotine has the formula </em>
<em> . To determine its composition, a sample is burned in excess oxygen, producing the following results:</em>
<em>Assume that all the atoms in nicotine are present as products </em>
<h2>Solution</h2>
To find the empirical formula you need to find the moles of C, H, and N in each of the compound.
- 1.0 mol of CO₂ has 1.0 mol of C
- 0.70 mol of H₂O has 1.4 mol of H
- 0.20 mol of NO₂ has 0.20 mol of N
Thus, the ratio of moles is:
Divide all by the smallest number: 0.20
Hence, the empirical formula is C₅H₇N
Find the mass of 1 mole of units of the empirical formula:
Total mass = 60g + 7g + 14g = 81g
Two moles of units of the empirical formula weighs 2 × 81g = 162g and three units weighs 3 × 81g = 243 g.
Thus, since the molar mass is between 150 and 180 g/mol, the correct molar mass is 162g/mol and the molecular formula is twice the empirical formula: C₁₀H₁₄N₂.
Answer:
5
Explanation:
It requires 20 chracters to fill this answer
I'm not 100% sure that this is right but I think D. is correct.
Answer:
The liquid level will rise in Side A and drop in Side B.
Step-by-step explanation:
The membrane is impermeable to sucrose, but permeable to sucrose and water.
<u> Side A </u> <u> Side B </u>
2 M sucrose 1 M sucrose
1 M glucose 2 M glucose
(a) Ignoring osmotic effects
The glucose will diffuse spontaneously from the side with higher concentration to that of lower concentration until equilibrium is established. There is no change in volume on either side.
At this point, we have
<u> Side A </u> <u> Side B </u>
2 M sucrose 1 M sucrose
1.5 M glucose 1.5 M glucose
=====
(b) With osmotic effects
The solute concentration on Side A is greater than on Side B.
Water will diffuse into Side A.
The liquid level will rise in Side A and drop in Side B.
Answer:
Approximately
(note that
.)
Explanation:
The molarity of a solution gives the number of moles of solute in each unit volume of the solution. In this
solution in water,
Let
be the number of moles of the solute in the whole solution. Let
represent the volume of that solution. The formula for the molarity
of that solution is:
.
In this question, the volume of the solution is known to be
. That's
in standard units. What needs to be found is
, the number of moles of
in that solution.
The molar mass (formula mass) of a compound gives the mass of each mole of units of this compound. For example, the molar mass of
is
means that the mass of one mole of
.
For this question,
.
Calculate the molarity of this solution:
.
Note that
(one mole per liter solution) is the same as
.