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prohojiy [21]
3 years ago
6

What is the osmotic pressure of a solution made by dissolving 75.0 g of glucose, c6h12o6, in enough water to form 700.0 ml of so

lution at 45.0 ∘c ? express your answer to three significant figures and include the appropriate u?
Chemistry
1 answer:
lions [1.4K]3 years ago
8 0
We will use the osmotic pressure formula:
π = n R T / V
When π is the osmotic pressure (atm)
n is no.of moles when the molar mass of glucose = 180 g/mol
so, n = 75 g / 180 g/mol= 0.42

and R is gas constant = 0.0821 L.atm/mol.k 
T is the temperature in Kelvin = 45 +273 = 318 K
and V is the volume in Litre = 700 / 1000 = 0.7 L
So, by substitution:
∴ π = 0.42 * 0.0821 * 318 / 0.7 = 15.665 atm
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The diagram below shows the atoms involved in forming table salt. Which statement best describes what happens next ?
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What is the oxidation number of nitrogen in the nitrate ion NO31−?
ahrayia [7]

In No3-1 the oxidation number of oxygen is -5 so oxidation number of N would be +5

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What is the theoretical yield of moles of hydrogen that can be produced from 0.032g of MG?
Ugo [173]

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1.31x10⁻³ moles of H₂

Explanation:

This is the equation:

Mg(s)  +   2H₂O (g)   →   Mg(OH)₂ (aq)   +    H₂(g)

Ratio is 1:1, so 1 mol of Mg is needed to produce 1 mol of H₂

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5 0
2 years ago
Calculate the number of grams of solute in 814.2mL of 0.227 M calcium acetate
kiruha [24]

Answer:

Mass = 29.23 g

Explanation:

Given data:

Volume of solution = 814.2 mL 814.2/1000 = 0.8142 L)

Molarity of solution = 0.227 M

Mass of solute in gram = ?

Solution:

Molarity = number of moles / volume in L

By putting values,

0.227 M = number of moles / 0.8142 L

Number of moles = 0.227 M × 0.8142 L

Number of moles = 0.184 mol

Mass in gram:

Mass = number of moles × molar mass

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Mass = 0.184 mol × 158.17 g/mol

Mass = 29.23 g

6 0
3 years ago
The accepted value for the molar volume of a gas is 22.4 L. Sarah's experimental data indicated that a mole of a gas had a volum
Amanda [17]

Answer:

Percent error = 12.5%

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In a measurement you can find percent error following the formula:

Percent error = |Measured value - Accepted Value| / Acepted value * 100

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Replacing:

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Percent error = |-2.8L| / 22.4L * 100

Percent error = 2.8L / 22.4L * 100

Percent error = 12.5%

3 0
3 years ago
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