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Natasha2012 [34]
3 years ago
10

Hydrogen gas has a density of 0.090 g/L, and at normal pressure and -1.72 C one mole of it takes up 22.4 L. How would you calcul

ate the moles in 900. g of hydrogen gas? Set up the math. But DONT DO ANY OF IT. Just leave your answer as a math expression.
Chemistry
2 answers:
FromTheMoon [43]3 years ago
8 0

Answer:

n = \frac{900}{0.090*22.4}

Explanation:

If 1 mole of hydrogen gas occupies 22.4 L, then, the number of moles of hydrogen gas (n) can be found by the volume (V):

1 mole ----- 22.4 L

n ------ V

By a simple direct three rule:

22.4n = V

n = V/22.4

But the volume is mass(m) divided by the density (d)

V = m/d

So

n = \frac{m}{22.4*d}

For a mass of 900 g and a density of 0.090 g/L:

n = \frac{900}{0.090*22.4}

BlackZzzverrR [31]3 years ago
6 0

Answer:

n= \frac{m}{ \rho }* \frac{1 mol}{22.4 L}

Explanation:

Assuming that all caculations are at normal pressure and -1.72°C :

n= \frac{m}{ \rho }* \frac{1 mol}{22.4 L}

Where

n is the number of moles of hydrogen

n is the mass of hydrogen

\rho is the density of hydrogen

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A gas has experienced a small increase in volume but has maintained the same pressure and number of moles. According to the idea
krek1111 [17]

Answer:

If a gas has experienced a small increase in volume but has maintained the same pressure and number of moles, the temperature of the gas will DROP.

Explanation:

According to Boyle’s law of ideal gases, volume and temperature of a gas is inversely related, as long as the pressure is kept constant;

P₁V₁/T₁ = P₂V₂/T₂

Therefore, if the volume of the gas increases, the temperature will definitely decrease due to the inverse relationship. The gas will get cooler.  

Learn More:

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#LearnWithBrainly

4 0
3 years ago
What is the mole fraction of ethanol when 10.00 ml of pure ethanol is combined with 2.00 ml of water? the volume of 10 ml of the
GenaCL600 [577]
The mole fraction is calculated using the formula:

mole fraction of component A = # of moles of component A / # of total moles of the solution.

A) number of moles of ethanol

To calculate the number of moles of ethanol, you need its density, which will permit you to determine the mass of the 10.00 ml, and then convert into moles using the molar mass of ethanol.

The normal density of ethanol is 0.789 g/ml

density = mass / volume => mass = density  * volume = 0.789 g/ml * 10.00 ml = 7.890 g

Molar mass of ethanol = 46.07 g/mol

number of moles = mass / molar mass = 7.890g / 46.07 g/mol = 0.1713 mol

B) number of moles of water

density of water = 1.00 g/mol

mass of water = density * volume = 1.00 g/mol * 2.00 ml = 2.00 g

number of moles of water = mass / molar mass = 2.00 g / 18.0 g/mol = 0.111  mol

C) mole fraction

mole fraction of ethanol = number of moles of ethanol / number of moles of solution

number of moles of ethanol = 0.1713 / (0.1713 + 0.111) = 0.1713 / 0.2824 = 0.607

Answer: 0.607

The volume of the final solution may  be calculated by adding the volume of the two components. This is 10.00 ml of ethanol + 2.00 ml of water makes 12.00 ml of solution.

It is not clear what the second question is meant for. Some context is missing. If you know density and you know maqss (or can calculate the mass from other data) you do not need to measure the volume.
3 0
3 years ago
Number 2 how many moles of propane (C3H8) are there in 6.2 g of propane? Correct answer will get brainliest.
skad [1K]
In 1 mole of propane, there are 44 grams
so, X moles = 6.2 grams
Cross multiply: 44x = 6.2
x = 0.14 moles
(In scientific notation) The answer is B
6 0
3 years ago
What is the vapor pressure of a solution in which the mole fraction of the solute is 0.200 and the vapor pressure of the pure so
Ulleksa [173]

Answer: The vapor pressure of a solution in which the mole fraction of the solute is 0.200 is 80.0 torr

Explanation:

As the relative lowering of vapor pressure is directly proportional to the amount of dissolved solute.

The formula for relative lowering of vapor pressure will be,

\frac{p^o-p_s}{p^o}=i\times x_2

where,

p^0= vapor pressure of pure solvent = 100.0 torr

p_s = vapor pressure of solution = ?

i = Van'T Hoff factor = 1 for nonvolatile, nonelectrolyte solute

x_2 = mole fraction of solute  = 0.200  

\frac{100.0-p_s}{100.0}=1\times 0.200

p_s=80.0torr

The vapor pressure of a solution in which the mole fraction of the solute is 0.200 is 80.0 torr

7 0
3 years ago
How can your knowledge of acids and bases
fenix001 [56]

Answer:

How can we make use of acids or bases to remove heavy metals from soils? We can remove heavy metals from soil by adding acid and catching the solution that drains through. Acids can react with metals turning metalic compounds which can be dissolved by water and washed away. Improve crop yields?

Explanation:

7 0
3 years ago
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