Question

a 500 mL container holds 2.76 g of oxygen at -26 C what is the gas pressure in mmHg

Answer 1

[AI-generated answer — Bot GPT 3.5]

To find the gas pressure, we can use the ideal gas law equation: PV = nRT.

First, we need to find the number of moles of oxygen in the container. We can use the formula n = m/M, where m is the mass of oxygen and M is the molar mass of oxygen (32 g/mol).

m = 2.76 g
M = 32 g/mol

n = 2.76 g / 32 g/mol = 0.08625 mol

Next, we need to convert the temperature from Celsius to Kelvin. We can do this by adding 273.15 to the temperature.

T = -26 C + 273.15 = 247.15 K

Now, we can substitute the values into the ideal gas law equation:

PV = nRT
P(500 mL) = (0.08625 mol)(0.0821 L·atm/mol·K)(247.15 K)
P(0.5 L) = 1.7225 L·atm/mol
P = 1.7225 L·atm/mol / 0.5 L = 3.445 atm

Finally, we can convert the pressure from atm to mmHg:

1 atm = 760 mmHg
3.445 atm * 760 mmHg/atm = 2617.2 mmHg

Therefore, the gas pressure in the 500 mL container at -26 C is 2617.2 mmHg.