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ioda
2 years ago
9

What is the mass of 187 liters of CO2 gas? The volume is measured at STP.

Chemistry
1 answer:
WITCHER [35]2 years ago
7 0

The mass of 187 liters of CO2 gas is 0.36 g.

<u>Explanation:</u>

The molecular weight of CO2 is 44 g / mol.

1 kg of CO2 = 1000 g \times ( 1 mole / 44 g) = 22.7 mole of CO2.

By using the ideal gas equation,

                                    PV = nRT

                                      V = nRT / P

where P represents the pressure,

          V represents the volume,

          T represents the temperature,

          R represents the ideal gas constant,

          n represents the amount of substance.

                                   V = (22.7)\times(0.0821)\times(273.15) / 1

                                   V = 509.6 L of CO2 at STP

            Mass = (187 L of CO2 gas) / (509.6 L of CO2 at STP)

                       = 187 / 509.6

            mass = 0.36 g

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A gas sample occupies a volume of 1.264 L when the temperature is 168.0 °C and the pressure is 946.6 torr. How many molecules ar
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Answer:

0.26×10²³ molecules

Explanation:

Given data:

Volume of gas = 1.264 L

Temperature = 168°C

Pressure = 946.6 torr

Number of molecules of gas = ?

Solution:

Temperature = 168°C (168+273= 441 K)

Pressure = 946.6 torr (946.6/760 = 1.25 atm)

Now we will determine the number of moles.

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

n = PV/RT

n = 1.25  atm ×1.264 L / 0.0821 atm.L/ mol.K   ×441 K

n = 1.58 /36.21 /mol

n = 0.044 mol

Now we will calculate the number of molecules by using Avogadro number.

1 mol = 6.022×10²³ molecules

0.044 mol × 6.022×10²³ molecules/ 1mol

0.26×10²³ molecules

5 0
2 years ago
A compound distributes between benzene (solvent 1) and water (solvent 2) with a distribution coefficient, K = 2.7. If 1.0g of th
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Explanation:

The given data is as follows.

Solvent 1 = benzene,          Solvent 2 = water

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V_{S_{1}} = 10 mL,       weight of compound = 1 g

       Extract = 3

Therefore, calculate the fraction remaining as follows.

                  f_{n} = [1 + K_{p}(\frac{V_{S_{2}}}{V_{S_{1}}})]^{-n}

                                  = [1 + 2.7(\frac{100}{10})]^{-3}

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Hence, weight of compound to be extracted = weight of compound - fraction remaining

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or,                               = 1 \times 10^{-5}

Thus, we can conclude that weight of compound that could be extracted is 1 \times 10^{-5}.

7 0
2 years ago
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O 1. 12 moles
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Answer:

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Explanation:

Hello there!

In this case, according to the given question about stoichiometry, it is possible for us to calculate the required moles of water that will be produced by 12 grams of hydrogen, by using the molar mass of this reactant (2.02 g/mol as it is diatomic) and the 2:2 mole ratio in the chemical equation by solving the following setup:

n_{H_2O}=12gH_2*\frac{1molH_2}{2.02gH_2} *\frac{2molH_2O}{2molH_2} \\\\n_{H_2O}=5.94molH_2O

Regards!

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