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igor_vitrenko [27]
2 years ago
8

Use the ideal gas law to calculate the pressure in atmospheres of 0.21 mol of helium (He) at 16°C & occupying 2.53 L. You mu

st show all of your work to earn credit. **Don't forget to convert your Celsius temperature to Kelvin**
*picture attached !!*

Chemistry
1 answer:
chubhunter [2.5K]2 years ago
4 0

Answer:

The answer to your question is 2.32 atm

Explanation:

Data

P = ?

n = 0.214

V = 2.53 L

T = 61°C

R = 0.082 atm L/mol°K

Formula

PV = nTR

solve for P

P = nRT/V

Process

1.- Calculate the temperature in K

°K = °C + 273

°K = 61 + 273

    = 334

2.- Substitution

P = (0.214 x 0.082 x 334) / 2.53

3.- Simplification

P = 5.86/2.53

4.- Result

P = 2.32 atm

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45.0 g of Ca(NO3)2 are used to create a 1.3 M solution. What is the volume of the solution
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As we know that Molarity is given as,

                                       M = moles / V 
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                                        V = moles / M ------------------(1)
Also, moles is equal to,
                                       moles = mass / M. mass -------------(2)
puting value of moles from eq. 2 into eq. 1,
                                       V = (mass / M.mass) / M
Putting values,
                                       V = (45 g / 164 g/mol) / 1.3 mol/dm³

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6 0
3 years ago
If 20.0 mL of glacial acetic acid (pure HC2H3O2HC2H3O2) is diluted to 1.70 L with water, what is the pH of the resulting solutio
Andreas93 [3]

Answer:

The answer to your question is pH = 0.686

Explanation:

Data

Acetic acid = 20 ml

Final volume = 1.7 L

pH = ?

density = 1.05 g/ml

Process

1.- Calculate the mass of acetic acid

density = mass / volume

mass = density x volume

mass = 1.05 x 20

mass = 21 g

2.- Calculate the moles of acetic acid (CH₃COOH)

Molar mass = (12 x 2) + (16 x 2) + (4 x 1)

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4.- Calculate the pH

pH = -log[0.206]

pH = 0.686

6 0
3 years ago
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