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What pressure, in Torr, will be exerted by 25.0g of CO2 at a temperature of 25.0 °C and a volume of 500.0 mL?

User Sadegh
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1 Answer

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To find the pressure exerted by 25.0 g of CO2 at a temperature of 25.0°C and a volume of 500.0 mL, we can use the ideal gas law:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

First, we need to convert the given temperature from Celsius to Kelvin by adding 273.15:

T = 25.0°C + 273.15 = 298.15 K

The molar mass of CO2 is 44.01 g/mol. To find the number of moles, we divide the mass by the molar mass:

n = m/M = 25.0 g / 44.01 g/mol ≈ 0.568 mol

Now we can plug in the given values and solve for P:

P = (nRT) / V = (0.568 mol x 0.0821 L atm mol^-1 K^-1 x 298.15 K) / 0.500 L

P = 22.6 atm

Finally, we can convert the pressure from atm to Torr by multiplying by 760:

P = 22.6 atm x 760 Torr/atm ≈ 17176 Torr

Therefore, the pressure exerted by 25.0 g of CO2 at a temperature of 25.0°C and a volume of 500.0 mL is approximately 17176 Torr.
User Imike
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