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Phoenix [80]
2 years ago
5

What is the volume, in milliliters, of 6.56 g of acetone?

Chemistry
1 answer:
PIT_PIT [208]2 years ago
4 0

Answer:

8.29 mL

Explanation:

Density of acetone in g/mL = 0.791 g/ml

Dimensional analysis: 6.56 g x (1 mL/0.791 g) = 8.29 mL

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statuscvo [17]

A. cellular function

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5 0
3 years ago
Calculate the mass, in grams, of cucl2 (mw = 134.452 g/mol) required to prepare 250.0 ml of a 6.11 % w/v cu2 (mw = 63.546 g/mol)
Sever21 [200]

6.11% w/v of Cu2+ implies that 6.11 g of Cu2+ is present in 100 ml of the solution

therefore,  250 ml of the solution would have: 250 ml * 6.11 g/100 ml = 15.275 g

# moles of Cu2+ = 15.275 g/63.546 g mole-1 = 0.2404 moles

1 mole of CuCl2 contain 1 mole of Cu2+ ion

Hence, 0.2404 moles of Cu2+ would correspond to 0.2404 moles of CuCl2

Molar mass of CuCl2 = 134.452 g/mole

The mass of CuCl2 required = 0.2404 moles * 134.452 g/mole = 32.32 grams

6 0
3 years ago
How much heat is required to increase the temperature of 35.0 grams of water from 10.0°C to 45.0°C? (The specific heat of water
kati45 [8]
Q = mCΔT
Q is heat in Joules, m is mass, C is the specific heat of water, delta T is the change in temperature

Q = (35g)(4.18)(35 degrees) = 5121 Joules or 5.12 kJ required


7 0
3 years ago
Read 2 more answers
The normal boiling point of a substance is defined to be the temperature at which the liquid phase of the substance is in equili
boyakko [2]

Answer:

ΔSv = 0.1075 KJ/mol.K

Explanation:

Binary solution:

∴ a: solvent

∴ b: solute

in equilibrium:

  • μ*(g) = μ(l) = μ* +RTLnXa....chemical potential (μ)

⇒ Ln (1 - Xb) = ΔG/RT

∴ ΔG = ΔHv - TΔSv

⇒ Ln(1 -Xb) = ΔHv/RT - ΔSv/R

∴ Xb → 0:

⇒ Ln(1) = ΔHv/RT - ΔSv/R

∴ T = T*b....normal boiling point

⇒ 0 = ΔHv/RT*b - ΔSv/R

⇒ ΔSv = (R)(ΔHv/RT*b)

⇒ ΔSv = ΔHv/T*b

∴ T*b = 80°C ≅ 353 K

⇒ ΔSv = (38 KJ/mol)/(353 K)

⇒ ΔSv = 0.1075 KJ/mol.K

5 0
3 years ago
While in Europe, if you drive 125 km per day, how much money would you spend on gas in one week if gas costs 1.10 euros per lite
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You would have spent $18.9
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3 years ago
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