Wiki User
∙ 7y agoThe volume of a gas can be calculated using the ideal gas law equation, (PV = nRT), where (P) is pressure, (V) is volume, (n) is the number of moles, (R) is the ideal gas constant, and (T) is temperature. Rearranging the equation to solve for volume gives us: (V = \frac{{nRT}}{P}). Plugging in the values, we get: (V = \frac{{2\ moles \times 0.0821\ L \cdot atm/mol \cdot K \times 300\ K}}{1.3\ atm} = 37.85\ L).
The molar volume of a gas at STP (standard temperature and pressure) is 22.4 L/mol. Therefore, the volume occupied by 2 moles of oxygen would be 44.8 L.
At room temperature and pressure, 1 mole of ideal gas occupies 22.4 liters. Therefore, 8.00 moles of oxygen will occupy 8.00 x 22.4 = 179.2 liters.
The partial pressure of oxygen can be calculated using the partial pressure formula: P(O2) = (moles of O2 / total moles) x total pressure. First, convert milliliters of gases into moles using the ideal gas law. Then, apply the formula to find the partial pressure of oxygen.
1 mole of gas at STP (Standard Temperature and Pressure) occupies 22.4 L. Therefore, 1.50 moles of CH4 at STP would occupy 33.6 L (1.50 moles x 22.4 L/mol).
Since there are 8 oxygen atoms in each molecule of C8H11NO2, you would have 29.6 moles of oxygen in 3.7 moles of C8H11NO2.
The molar volume of a gas at STP (standard temperature and pressure) is 22.4 L/mol. Therefore, the volume occupied by 2 moles of oxygen would be 44.8 L.
38 L
38 L
At room temperature and pressure, 1 mole of ideal gas occupies 22.4 liters. Therefore, 8.00 moles of oxygen will occupy 8.00 x 22.4 = 179.2 liters.
The equivalent in moles is 6,03.
The partial pressure of oxygen can be calculated using the partial pressure formula: P(O2) = (moles of O2 / total moles) x total pressure. First, convert milliliters of gases into moles using the ideal gas law. Then, apply the formula to find the partial pressure of oxygen.
The volume of a gas depends on its pressure, temperature, and volume according to the ideal gas law PV = nRT. Without knowing the pressure, temperature, or container size, it's not possible to determine the volume occupied by the 0.48 moles of hydrogen.
The partial pressure of oxygen is 128 kPa.
1 mole of gas at STP (Standard Temperature and Pressure) occupies 22.4 L. Therefore, 1.50 moles of CH4 at STP would occupy 33.6 L (1.50 moles x 22.4 L/mol).
To determine the number of moles of nitrogen and oxygen in a given volume like a cubic foot, you would first need to know the pressure and temperature of the gas. Then you can use the ideal gas law equation, PV = nRT, where P is pressure, V is volume, n is moles, R is the ideal gas constant, and T is temperature. So without knowing the pressure and temperature, it is not possible to determine the number of moles of nitrogen and oxygen in a cubic foot.
Using Henry's law, the number of moles of oxygen that will dissolve is calculated by multiplying Henry's constant by the partial pressure of oxygen and the volume of water. So, moles of oxygen = 0.0013 mol L ATM * 0.21 ATM * 45 L = 0.1233 mol of oxygen will dissolve in 45 L of water at 20C.
Since there are 8 oxygen atoms in each molecule of C8H11NO2, you would have 29.6 moles of oxygen in 3.7 moles of C8H11NO2.