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shusha [124]
3 years ago
5

Does carbon dissolve in water

Chemistry
1 answer:
Damm [24]3 years ago
5 0

Answer:

yes

Explanation:

CO2 is soluble because water molecules are attracted to these polar areas. The bond between carbon

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a gas is contained in a thick walled balloon. when the pressure changes from 417 mm hg to 576 mm hg, the volume changes from l t
melomori [17]
We can use the combined gas law equation to solve for the initial volume
\frac{P1V1}{T1} =  \frac{P2V2}{T2}
parameters for the first instance are on the left side and parameters for the second instance are on the right side of the equation 
substituting the values in the equation 
\frac{417 mmHg*V}{497 K} =  \frac{576mmHg*4.78L}{386K}
V = 8.50 L
the initial volume is 8.50 L
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Select all that apply: Select the benefits of sexual reproduction.
malfutka [58]
Sexual reproduction promotes adaptations, increases genetic diversity, and increases chances of survival. 
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3 years ago
Write the chemical formula for a molecule of non cyclic amp.
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6 0
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
How many ATOMS of boron are present in 3.61 grams of boron trifluoride ?
jeka57 [31]

Answer:

To determine the number of atoms of Boron that are present within 3.61 grams of Boron Trifluoride, it would be best to convert the grams to moles of the compound and then after that use the Avogadro's number to determine the number of molecules and then use the 1 to 3 ratio to determine the total number of Boron atoms.

5 0
2 years ago
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