What volume will be occupied by 33.0 grams of CO2 at 500 torr and 27 °C?

The volume that will be occupied by 33.0 grams of CO2 at 500 torr and 27 °C is 28.11L.

The volume of an ideal gas can be calculated using the ideal gas law equation as follows:

PV = nRT

Where;

According to this question;

0.657 × V = 0.75 × 0.0821 × 300

0.657V = 18.4725

V = 18.4725 ÷ 0.657

V = 28.11L

Therefore, the volume that will be occupied by 33.0 grams of CO2 at 500 torr and 27 °C is 28.11L.

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V = 27.98 L

Explanation:

Given data:

Mass of CO₂ = 33.0 g

Pressure = 500 torr

Temperature = 27°C

Volume occupied = ?

Solution:

Number of moles of CO₂:

Number of moles = mass/molar mass

Number of moles = 33.0 g/ 44 g/mol

Number of moles = 0.75 mol

Volume of CO₂:

PV = nRT

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

Now we will convert the temperature.

27+273 = 300 K

Pressure = 500 /760 = 0.66 atm

By putting values,

0.66 atm×V = 0.75 mol × 0.0821 atm.L/ mol.K  × 300 K

V = 18.47 atm.L/0.66 atm

V = 27.98 L

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calculate how many grams of ammonia can be produced from 4.21 grams of

n2 + 3h2 = 2nh3

my answer:

25.0g n2 x (1 mol/ 28.0gn2) x (2 mol nh3/ 1 mol n2) x (17.0g nh3/ 1 molnh3) = 30.36g n2

25.0g h2 x (1 mol h2/ 2.00g h2) x (2 mol nh3/ 3 mol h2) x (17.0g nh3/ 1 mol nh3) = 141.67g h2

lr = n2