Answer:
To calculate the density of carbon dioxide gas at a pressure of 0.936 atm and a temperature of 57°C, we can use the ideal gas law equation, which is 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. We can rearrange this equation to solve for the density, which is given by d = (PM) / (RT), where d is the density, P is the pressure, M is the molar mass of carbon dioxide, R is the gas constant, and T is the temperature in Kelvin. Since the temperature is given in Celsius, we need to convert it to Kelvin by adding 273.15. The molar mass of carbon dioxide is 44.01 g/mol.
Using the above equation, we get:
d = (0.936 atm * 44.01 g/mol) / ((0.0821 Latm/molK) * (57°C + 273.15))
d = 1.97 g/L
Therefore, the density of carbon dioxide gas at a pressure of 0.936 atm and a temperature of 57°C is 1.97 g/L.