Вопрос школьника
Gas at 15 ° C and a pressure of 760 mm Hg.Art. occupies a volume 2 liters. Bring the volume gas to normal conditions .
Ответ от учителя
To bring the volume of gas to normal conditions, we need to use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in Kelvin.
First, we need to convert the temperature from Celsius to Kelvin by adding 273.15. So, the temperature is 15 + 273.15 = 288.15 K.
Next, we need to find the number of moles of gas. We can use the formula n = PV/RT, where P, V, and T are the initial conditions (15 °C and 760 mm Hg) and R is the gas constant (0.0821 L·atm/mol·K).
n = (760 mm Hg) x (2 L) / (0.0821 L·atm/mol·K x 288.15 K)
n = 0.105 mol
Now, we can use the ideal gas law to find the volume of gas at normal conditions, which is defined as 0 °C (273.15 K) and 1 atm (760 mm Hg).
V = nRT/P
V = (0.105 mol) x (0.0821 L·atm/mol·K x 273.15 K) / 1 atm
V = 2.44 L
Therefore, the volume of gas at normal conditions is 2.44 liters.
