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What else can I help you with?
What is the volume of 3.5mol of CO2 gas at STP?
The volume of gas that 3.5 moles of oxygen occupy can be easily found using the relationship of PV=nRT where P is the pressure, V is the volume, n is the moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
How do I convert 76.0 grams of C4H10 to liters?
First, find out what the temperature and pressure of the gas is. Next, determine the mass per mole - this one I'll give you, it's 58.12 grams per mole. Divide 76 by 58.12 to get the number of moles of gas you have. Then, use the ideal gas law to determine the number of liters of gas per mole at the temp and pressure your gas is. Finally, multiply the liters per mole by the number of moles you have, and you've got it.
How many liters are in 1 ATM?
1 ATM (atmosphere) is a unit of pressure, not volume, so it does not directly correspond to liters. However, at standard temperature and pressure (STP), 1 ATM is equivalent to 1.01325 x 10^5 pascals, which is the same as 101.325 kilopascals (kPa). At STP, 1 mole of any ideal gas occupies approximately 22.4 liters, regardless of the pressure.
Calculate the mass of nitrogen dissolved at room temperature in an 96.0 home aquarium Assume a total pressure of 1.0 and a mole fraction for nitrogen of 0.78?
Using Henry's Law /// Solubility=(constant) (Pressure) We know that the mole fraction is equal to the partial pressure, so (.78atm) The constant at room temp, (from table) 6.1*10^-4 (M/atm) solubility = (6.1*10^-4)(.78) =4.758*10^-4 M So you just take your solubility (moles/L) x 92L to give you the number of moles =0.438moles times the g/mole of Nitrogen (N2) which is 28g/mol =1.2g I don't really understand how the other person did theirs, but I did not want to delete it, so it goes as follows: ______________________________________ .78/92=.84782 .84782 x 14.01= .11878 Move the decimal one over to the right. Answer= 1.2
At STP 0.250L of an unknown gas has a mass of 1.00 gram. Calculate its molar mass.?
1 standard volume of 1 mole of any gas @ STP is 22.4 LSo the # of moles in a 1 L sample will be:1 L*(1 mol/22.4 L) = 0.04464 molSince you already know the mass of the gas @ STP, the molar mass will be mass/#moles1.92 g/ 0.04464 mol = 43.01 g/mol
If the ideal gas constant has a volume of 0.0821 what are the units?
The ideal gas constant ( R ) with a value of 0.0821 has units of liters·atmospheres per mole·kelvin (L·atm/(mol·K)). This means it describes how much volume one mole of an ideal gas occupies at standard temperature and pressure. The units reflect the relationship between pressure, volume, temperature, and the amount of substance in the ideal gas law equation, ( PV = nRT ).
If the temperature of a gas is constant and you multiply its pressure by its volume it will always equal the what?
Ideal gas Law PV = nRT where P is pressure V is volume n is moles R is a constant of 8.31 and T is temperature so if u multiply PV with T constant, that leaves nR, therefore you will always get mole of the air multiplied with 8.31
What are the four variables in the ideal gas law?
The four variables in the ideal gas law are pressure (P), volume (V), temperature (T), and the number of moles of gas (n). These variables are related by the equation PV = nRT, where R is the ideal gas constant.
Which correctly defines molar volume of an ideal gas?
The molar volume of an ideal gas is defined as the volume occupied by one mole of the gas at standard temperature and pressure (STP), which is 0°C (273.15 K) and 1 atm pressure. Under these conditions, the molar volume is approximately 22.4 liters. This value is derived from the ideal gas law, which states that 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.
When a mole of gas occupies 22.4 Liters this is known as?
This is the molar volume of an ideal gas at a given temperature and pressure.
What is the constant for 1 mole of any ideal gas?
The Universal Gas Constant is 8.314 J/K/Mole
What is constant for 1 mole of any ideal gas?
The Universal Gas Constant is 8.314 J/K/Mole
What is the volume of a mole of any gas at standard temperature and pressure?
The volume of a mole of any gas at Standard Temperature and Pressure (STP) is approximately 22.4 liters. This is known as the molar volume of a gas at STP and is a standard value used in gas calculations.
At a constant temperature the pressure exerted by one mole of a gas decreases if the volume available is increased?
Yes, according to Boyle's Law, at a constant temperature, the pressure of a gas is inversely proportional to its volume. This means that if the volume available to the gas is increased, the pressure exerted by the gas will decrease.
If the volume of mole of gas molecules remains constant lowering the temperature will make the pressure?
If the volume of a mole of gas molecules remains constant and the temperature is lowered, the pressure of the gas will decrease. This relationship is described by Gay-Lussac's law, which states that the pressure of a gas is directly proportional to its absolute temperature when volume is held constant. As temperature drops, the kinetic energy of the gas molecules decreases, resulting in fewer collisions with the walls of the container and thus lower pressure.
A metal cylinder contains 1 mol of nitrogen gas what will happen to the pressure if another mole of gas is added to the cylinder but the temperature and volume do not change?
The addition of another mole of gas will double the number of gas molecules in the cylinder, leading to a doubling of the pressure according to Avogadro's law, which states that at constant temperature and volume, the pressure of an ideal gas is directly proportional to the number of moles of gas present.
What volume does 1 mole of diatomic gas particles occupy at NTP?
At NTP (normal temperature and pressure), 1 mole of any gas occupies approximately 24 liters of volume. This is due to the ideal gas law, which relates the volume, pressure, temperature, and amount of gas.
