Calculate the pressure exerted by 1.5g of co2 gas at temperature of 35°c and a volume of 525cm³ ? [ choose the appropriate R value ]

Answer 1

To calculate the pressure exerted by the CO2 gas, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume (convert cm^3 to L by dividing by 1000)
n = number of moles of gas
R = ideal gas constant
T = temperature in Kelvin (add 273 to Celsius temperature)

First, we need to calculate the number of moles of CO2 gas:

molecular weight of CO2 = 12.01 (C) + 2 * 16.00 (O) = 44.01 g/mol

1.5g of CO2 x (1 mol CO2 / 44.01 g) = 0.034 mol CO2

Next, convert the volume to liters:

V = 525 cm^3 / 1000 = 0.525 L

Now, convert the temperature to Kelvin:

T = 35°C + 273 = 308 K

Now, we can determine the pressure using the formula with the appropriate value of the ideal gas constant R:

We can use the value R = 0.0821 L•atm/mol•K for units of pressure in atm:

P = (0.034 mol) * (0.0821 L•atm/mol•K) * (308 K) / 0.525 L
P ≈ 1.706 atm

Therefore, the pressure exerted by 1.5g of CO2 gas at a temperature of 35°C and a volume of 525 cm^3 is approximately 1.706 atm when using the value of R = 0.0821 L•atm/mol•K.