the correct number of significant digits
addition= -3.220g = 4 significant digits.
subtract= -5.820g = 4 significant digits
<h3>How are significant digits determined?</h3>
- Use the following three rules to determine how many significant figures are present in a number:
- Digits that are not zero are always important. Any zeros in the range of two significant digits are noteworthy.
- ONLY in the decimal section are a final zero or following zeros important.
<h3>What are examples of significant digits?</h3>
- Any two non-zero digits that are separated by a zero are important. For instance, the number 108.0097 has seven significant digits.
- Every zero that is both to the right and left of a non-zero digit and the decimal point is never meaningful.
- For instance, the number 0.00798 had three significant digits.
learn more about significant digits here
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Answer:
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Answer:
23.4 torr
Explanation:
For solutions that contain non-volatile solutes, the vapor pressure of the solution can be determined by using the mole fraction of the solvent and the vapor pressure of the pure solvent at the same temperature.
P
sol
=
χ
solvent
⋅
P
∘
solvent
, where
P
sol
is the vapor pressure of the solution
χ
solvent
is the mole fraction of the solvent
P
∘
solvent
is the vapor pressure of the pure solvent
In your case, you know that the vapor pressure of pure water at
25
∘
C
is equal to
23.8
torr. This means that all you have to do is determine the mole fraction of water in the solution.
As you know, mole fraction is defined as the number of moles of a component of a solution divided by the total number of moles present in that solution.
Use glucose and water's respective molar masses to determine how many moles of each you have
18.0
g
⋅
1 mole glucose
180.0
g
=
0.100 moles glucose
and
95.0
g
⋅
1 mole water
18.015
g
=
5.273 moles water
The total number of moles present in the solution will be
n
total
=
n
glucose
+
n
water
n
total
=
0.100
+
5.273
=
5.373 moles
This means that the mole fraction of water will be
χ
water
=
5.273
moles
5.373
moles
=
0.9814
Finally, the vapor pressure of the solution will be
P
sol
=
0.9814
⋅
23.8 torr
=
23.4 torr
The answer is rounded to three sig figs.
Answer:
760.39 mmHg (approx.)
Explanation:
Okay so given the first set of information, we have:
T = 406 K (133+273)
V = 20 L
P = 1.1184 atm (converted for continuity reasons from mmHg)
R = 0.08206 L atm/mol K
Using PV = nRT (ideal gas law), we solve for n (moles of SO2).
n = PV/RT = (1.1184 atm * 20 L) / (0.08206 L atm/mol K * 406 K) = 0.6714 mol
Now that you have all the information, you can use the new volume and temperature to solve for pressure.
T = 454 K (181+273)
V = 25 L
n = 0.6714 mol
R = 0.08206 L atm/mol K
Using the ideal gas law again, we solve for P (pressure in <u>atm</u>).
P = nRT/V = (0.6714 mol * 0.08206 L atm/mol K * 454 K) / (25 L) = 1.0005 atm
Then we convert atm back to mmHg to get 760.39 mmHg.