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wel
3 years ago
8

How many quarters fit in a 1.75 liter bottle?

Chemistry
2 answers:
WARRIOR [948]3 years ago
8 0
1.85 quarts can fit into a 1.75 liter bottle
Volgvan3 years ago
3 0

Answer:

In a 1.75 liter bottle fit 1.8492 quarters.

Explanation:

The quarter is a unit of volume. It is equivalent to \frac{1}{4} of a gallon :

1gallon=3.78541L

Where L is liter

⇒

\frac{1}{4}gallon=1quarter=\frac{3.78541L}{4}

To find how many quarters fit in a 1.75 L bottle we can write :

\frac{\frac{3.78541L}{4}}{1quarter}=\frac{1.75L}{x}

Solving for x :

x=\frac{(1.75L).(1quarter)}{\frac{3.78541L}{4}}

x=1.8492quarters

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3 years ago
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3 years ago
Mass of metal=0.0291. Volume of gas collected over water=25.67mL. Temperature=24.1C. Atmospheric pressure=754.6mmHg. Note: Metal
NISA [10]

Answers:

1) 732.1 mmHg; 2) 0.001 014 mol; 3) 0.001 014 mol; 4) 28.7 g/mol; 5) 187 ppt.

Explanation:

1) <em>Partial pressure of hydrogen</em>

You are collecting the gas over water, so

p_{\text{atm}} = p_{\text{H}_{2}} + p_{\text{H}_{2}\text{O}}

p_{\text{H}_{2}} = p_{\text{atm}} - p_{\text{H}_{2}\text{O}}

p_{\text{atm}} = \text{754.6 mmHg}

At 24.1 °C, p_{\text{H}_{2}\text{O}} = \text{22.5 mmHg}

p_{\text{H}_{2}} = \text{754.6 mmHg} - \text{22.5 mmHg} = \textbf{732.1 mmHg}

===============

2) Moles of H₂

We can use the Ideal Gas Law.

<em>pV = nRT</em>                Divide both sides by <em>RT</em> and switch

<em>n</em> = (<em>pV</em>)/(<em>RT</em>)

p = 732.1 mmHg                                                 Convert to atmospheres

p = 732.1/760                                                      Do the division

p = 0.9633 atm

V = 25.67 mL                                                        Convert to litres

V = 0.025 67 L

R = 0.082 06 L·atm·K⁻¹mol⁻¹

T = 24.1 °C                                                              Convert to kelvins

T = (24.1 + 273.15 ) K = 297.25 K                          Insert the values

n = (0.9633 × 0.025 67)/(0.082 06 × 297.25)     Do the multiplications

n = 0.02473/24.39                                                 Do the division

n = 0.001 014 mol

===============

3)<em> Moles of metal </em>

The partial chemical equation is

M + … ⟶ H₂ + …

The molar ratio of M:H₂ is 1 mol M:1 mol H₂.

Moles of M = 0.001 014 × 1/1                          Do the operations

Moles of M = 0.001 014 mol M

===============

4) Atomic mass of M

Atomic mass = mass of M/moles of M     Insert the values

Atomic mass = 0.0291/0.001 014             Do the division

Atomic mass = 28.7 g/mol

===============

5) <em>Relative deviation in ppt </em>

Your metal must be in Group 2 because of the 1:1 molar ratio of M:H₂.

The metal with the closest atomic mass is Mg (24.305 g/mol).

Relative deviation in ppt = |Experimental value – Theoretical value|/Theoretical value × 1000

Relative deviation = |28.7 – 23.405|/23.405 × 1000     Do the subtraction

Relative deviation = |4.39|/23.405 × 1000                      Do the operations

Relative deviation = 187 ppt

3 0
3 years ago
A sample of Xe takes 75 seconds to effuse out of a container. An unknown gas takes 60 seconds to effuse out of the identical con
miss Akunina [59]

Answer:

Kr

Explanation:

Now we have to apply Graham's law of diffusion in gases

t1/t2 = √M1/M2

If t1 is the time of diffusion of Xe = 75 seconds

t2 is the time of diffusion of the unknown gas = 60 seconds

M1= molar mass of Xe=131.293

M2= molar mass of the unknown gas

Thus;

75/60 = √131.293/M2

(75/60)^2= (√131.293/M2)^2

5625/3600=131.293/M2

M2= 3600×131.293/5625

M2= 84.0

The unknown gas is krypton (Kr)

8 0
3 years ago
Read 2 more answers
Data
Kitty [74]

Answer:

The 2nd one

Explanation: U answered yourself on the second one

3 0
3 years ago
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