how much pressure does 35 grams of carbon dioxide at 400 kelvin exert?
Use PV = nRT. n = g/molar mass. T is in Kelvin.
i think this question is correct. we cant calculate the volume. since we it is not in s.t.p.
To determine the pressure exerted by 35 grams of carbon dioxide at 400 Kelvin, you need to use the Ideal Gas Law equation: PV=nRT, where P represents pressure, V represents volume, n represents the number of moles, R is the ideal gas constant, and T is temperature in Kelvin.
To solve for pressure, we need to know the volume and number of moles. However, you have only provided the mass of carbon dioxide. Therefore, we need to convert the mass into moles using the molar mass of carbon dioxide.
The molar mass of carbon dioxide (CO2) is approximately 44 grams/mole since carbon has a molar mass of 12 grams/mole and oxygen has a molar mass of 16 grams/mole.
To convert 35 grams of carbon dioxide to moles, we divide the mass by the molar mass:
35 grams CO2 / 44 grams/mole = 0.795 moles CO2 (rounded to three decimal places)
Now, with the number of moles known, we can calculate the pressure. Plug in the values into the Ideal Gas Law equation:
P * V = n * R * T
Assuming the volume is constant (since you have not provided it), say V = 1 Liter, we can rearrange the equation:
P = (n * R * T) / V
Using the values:
n = 0.795 moles CO2
R = ideal gas constant ≈ 0.0821 L·atm/mol·K
T = 400 K
V = 1 L
P = (0.795 moles * 0.0821 L·atm/mol·K * 400 K) / 1 L
P ≈ 26.6 atm (rounded to two decimal places)
Therefore, 35 grams of carbon dioxide at 400 Kelvin exerts approximately 26.6 atmospheres of pressure.