Answer :
According to the given statement the mass of carbon in grams present in a 355 mL can at 5.0°C and 101.3 kPa is approximately 0.185 g.
To determine the mass of carbon in grams present in a 355 mL can at 5.0°C and 101.3 kPa, we need to follow these steps:
1. Convert the volume to liters: 355 mL = 0.355 L
2. Use the Ideal Gas Law formula: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant (8.314 J/mol·K), and T is the temperature in Kelvin.
3. Convert the temperature to Kelvin: 5.0°C + 273.15 = 278.15 K
4. Calculate the number of moles (n): n = PV/RT = (101.3 kPa × 0.355 L) / (8.314 J/mol·K × 278.15 K)
Since 1 kPa = 1000 Pa and 1 J = 1 N·m, we can convert the units:
n = (101300 Pa × 0.355 m³) / (8.314 N·m/mol·K × 278.15 K)
5. Solve for n: n ≈ 0.0154 mol
6. Calculate the mass of carbon: mass = n × molar mass of carbon
The molar mass of carbon is 12.01 g/mol, so the mass is:
mass = 0.0154 mol × 12.01 g/mol ≈ 0.185 g
The mass of carbon in grams present in a 355 mL can at 5.0°C and 101.3 kPa is approximately 0.185 g.
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