Molarity
The molarity of Na+ can be calculated by first converting the concentration from ppm to mol/L. Given that 1000 ppm is equivalent to 1000 mg/L, for Na+ (sodium ion) with a molar mass of approximately 23 g/mol, the concentration in mol/L is 1000 mg/L / 23 g/mol = 43.48 mmol/L. Converting this to mol/L gives 0.04348 M.
The molar volume of an ideal gas at standard temperature and pressure (STP) is 22.4 L/mol. Therefore, 0.75 mol of methane gas would occupy 16.8 liters (0.75 mol x 22.4 L/mol = 16.8 L).
The molar volume of a gas at standard temperature and pressure (STP) is 22.4 L/mol. Therefore, the volume of 2 moles of oxygen gas at STP would be 2 moles * 22.4 L/mol = 44.8 L.
This statement is true. According to the ideal gas law, at 0°C and 1 atm pressure, 1 mol of any ideal gas occupies 22.4 L of volume. Therefore, 1.0 mol of nitrogen would occupy 22.4 L and 2.0 mol of hydrogen would occupy 44.8 L in a 22.4 L box.
The molarity of a solution is calculated by dividing the number of moles of solute by the volume of the solution in liters. In this case, since the volume is 450 ml (0.45 L) and the number of moles of NaCl is 4.2 mol, the molarity would be 4.2 mol / 0.45 L = 9.33 M.
The molarity of Na+ can be calculated by first converting the concentration from ppm to mol/L. Given that 1000 ppm is equivalent to 1000 mg/L, for Na+ (sodium ion) with a molar mass of approximately 23 g/mol, the concentration in mol/L is 1000 mg/L / 23 g/mol = 43.48 mmol/L. Converting this to mol/L gives 0.04348 M.
The molar volume of an ideal gas at standard temperature and pressure (STP) is 22.4 L/mol. Therefore, 0.75 mol of methane gas would occupy 16.8 liters (0.75 mol x 22.4 L/mol = 16.8 L).
The molar volume of a gas at standard temperature and pressure (STP) is 22.4 L/mol. Therefore, the volume of 2 moles of oxygen gas at STP would be 2 moles * 22.4 L/mol = 44.8 L.
This statement is true. According to the ideal gas law, at 0°C and 1 atm pressure, 1 mol of any ideal gas occupies 22.4 L of volume. Therefore, 1.0 mol of nitrogen would occupy 22.4 L and 2.0 mol of hydrogen would occupy 44.8 L in a 22.4 L box.
mol/l
The molarity of a solution is calculated by dividing the number of moles of solute by the volume of the solution in liters. In this case, since the volume is 450 ml (0.45 L) and the number of moles of NaCl is 4.2 mol, the molarity would be 4.2 mol / 0.45 L = 9.33 M.
The volume of 0.0100 mol of CH4 gas at STP (Standard Temperature and Pressure) is 224 mL. This is based on the ideal gas law and the molar volume of a gas at STP, which is 22.4 L/mol. Converting this to milliliters gives 224,000 mL/mol.
202.44
The concentration of the solution is measured in moles per liter (mol/L).
Since you have you're Molarity and your Liters you can use the formula M= mol/ L 2.3 M = mol / .538 L Multiply both sides by .538 to get the mol alone. mol of KCL = 1.2374
4.25 grams. .050 M = .050 mol/1 L 5.0 L x .050 mol/L (cancel out L to get mol as a unit)= .25 mol Atomic mass of Ammonia (NH3)= 17 g/mol .25 mol x 17 g/mol (cancel out mol to get g as a unit)= 4.25 g
To find the number of moles of Ba(OH)2 present, we first need to calculate the amount of substance using the provided concentration and volume. This is done using the formula: moles = concentration (mol/L) x volume (L). Converting 205 mL to liters (205 mL = 0.205 L) and plugging in the values, we get moles = 0.600 mol/L x 0.205 L = 0.123 moles of Ba(OH)2.