To find the volume of 19.87 mol of NH₄Cl at STP (standard temperature and pressure), we can use the ideal gas law. At STP, 1 mol of gas occupies 22.4 L. Therefore, 19.87 mol of NH₄Cl will occupy 19.87 mol x 22.4 L/mol = 445.888 L.
To calculate the volume of a gas at STP (Standard Temperature and Pressure), you can use the ideal gas law equation: PV = nRT. At STP, the pressure is 1 atm, the temperature is 273 K, and the molar volume of an ideal gas is 22.4 L/mol. Plugging in the values, you can calculate the volume of 1.50 mol of Cl2 at STP.
The balanced chemical equation for the reaction is 2Mg + O2 -> 2MgO. This means that 1 mol of Mg will react with 0.5 mol of O2 to form 1 mol of MgO. The molar mass of Mg is 24 g/mol and MgO is 40 g/mol. Therefore, 12 g of Mg will require 3 mol of O2 (3 * 32 g) for complete conversion to MgO.
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 volume of 1 mol of gas at STP (standard temperature and pressure) is 22.4 L. Therefore, the volume of 2.22 mol of O2 at STP would be 2.22 mol x 22.4 L/mol = 49.7 L.
1 mol of any gas has a volume of 22.4 L at STP
The equation you will need is: Mol of substance 1 * volume of substance 1 = Mol of substance 2 * volume of substance 2
The quantity of gas in a given volume can be determined by two important gas equations. PV=nrT relates pressure and volume to the Ideal Gas Law constant, the amount of moles of gas and the system temperature. Once the system of the pressure (in atms), temperature (degrees Kelvin), gas constant (.0821 L*atm*K^-1*mol*-1), and volume (L) are known gas quantity in moles can be calculated.
This is the necessary heat to raise the temprataure of 1 mol with 1 kelvin, at constant volume.
When gasoline is heated in the presence of hydrogen gas and a catalyst, the gasoline crack. The cracking gasoline decomposes to 1 mol of methane, 2 mol of ethane, and 1 mole of propane for jet fuel. It is a process known as hydrocracking.
The molar volume at 1 bar and 0 0C is 22,710 980(38) L/mol; each mol contain 6,022 140 857.10e23 molecules.
3.0 kJ × 1 mol/40.65 kJ× 18.02 g/mol × 1 mL/1 g= 1.3 mL
The volume of any gas at STP is 22.4 liters/mole. Thus, 41.6 moles x 22.4 L/mole = 931.84 liters, or932 liters (to 3 sig figs).
16 a.m.u or 16 g mol-1
The volume is 50 %.
Solutions get diluted whenever there is an increase on volume but the number of moles of your substance remains the same. Eg: if I have 1 mole of NaCl in 1000ml, then I add 1000ml of water, then net volume is 2000ml but the number of moles of NaCl present is still 1 so the conc went from 1 mol/L to 0.5 mol/L. It was diluted!
Assuming that this ammonia gas is at STP, you can use Avogadro's number to gind the number of moles of gas:(387 x 1021 molecules) x (1 mol / 6.02x1023particles) x (17.03 g / 1 mol) =110 g NH3