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If the temperature of a fixed amount of gas is increased at a constant pressure what will happen to a volume?
Volume will increase. Think of it this way. If you heat a gas, it gets hotter. When a gas gets hotter, the atoms/molecules are "more active" and the pressure and/or the volume will go up. If your experiment with heating this gas sample must have a constant pressure, then volume will have to increase to give all those "more active" atoms/molecules more play room to prevent the pressure from going up.
What is the volume occupied by 26.9g of argon gas at a pressure of 1.23 and a temperature of 374?
To calculate the volume of the gas, you would need the ideal gas law equation: PV = nRT. First, convert grams of argon to moles using the molar mass of argon. Then, plug the values of pressure (P), temperature (T), and gas constant (R) into the equation with the calculated number of moles (n) to solve for volume (V).
What is the volume occupied by 10.7g of argon gas at apressure of 1.1 ATM and a temperrature of 448K?
Using the ideal gas law equation PV = nRT, where P is pressure, V is volume, n is number of moles, R is the ideal gas constant, and T is temperature, we can calculate the volume of gas. First, calculate the number of moles of argon using the given mass and molar mass of argon. Then, plug in the values into the equation to solve for volume. The volume of 10.7g of argon gas at 1.1 ATM and 448K is approximately 2.7 L.
Why volume of gas decreases on increasing pressure on it at constant temperature?
It is possible to explain this mathematically in terms of the Ideal Gas Laws, however, it should also be intuitively obvious that this is what would happen; when you press on a flexible substance, it compresses. This is equivalent to asking, why is it that when you push on a spring, you can make it shorter. Force moves things. How do you put pressure on a gas? You put it in a cylinder (such as the cylinder in an internal combustion engine) with a movable piston, and then you push the piston downward. Obviously, squeezing the gas will decrease its volume in the cylinder. The point about the constant temperature is that if you do this but the gas heats up, then the gas is going to push back. Again, this is what we see in an internal combustion engine. You compress the gas, but then there is fuel burned inside the cylinder, the gas gets very hot, and the piston is forced upward with considerable strength. So the engine runs.
What is the Reduction in volume of a substance due to pressure?
The reduction in volume of a substance due to pressure is described by Boyle's Law, which states that the volume of a gas decreases as pressure increases, assuming temperature remains constant. In other words, as pressure on a gas increases, the gas molecules are forced closer together, reducing the volume occupied by the gas.
What volume is occupied by 2.0g He at 25 degrees celsius and 775 mmHg?
A fixed quantity of gas at a constant pressure exhibits a temperature of 27 degrees Celsius and occupies a volume of 10.0 L. Use Charles's law to calculate: the temperature of the gas in degrees Celsius in atmospheres if the volume is increased to 16.0 L
How do you calculate the dissociation constant (Kd) from a binding curve?
To calculate the dissociation constant (Kd) from a binding curve, you can determine the concentration of ligand at which half of the binding sites are occupied. This concentration is equal to the Kd value.
When the pressure on a gas increases at constant temperature its volume?
decreases
How can you calculate cost per occupied room?
You can calculate the cost per occupied room by evaluating all of the costs of each occupied room such as the cost of cleaning, maintenance or repairs. The addition of all of these costs together will give you the cost per occupied room in your building.
If the temperature of a fixed amount of gas is increased at a constant pressure what will happen to a volume?
Volume will increase. Think of it this way. If you heat a gas, it gets hotter. When a gas gets hotter, the atoms/molecules are "more active" and the pressure and/or the volume will go up. If your experiment with heating this gas sample must have a constant pressure, then volume will have to increase to give all those "more active" atoms/molecules more play room to prevent the pressure from going up.
How do you calculate the density of matter?
Volume occupied divided by weight
How do you calculate KD from a binding curve?
To calculate the dissociation constant (KD) from a binding curve, you can use the equation KD C50, where C50 is the concentration of the ligand at which half of the binding sites are occupied. This value can be determined by plotting the binding data and finding the point where half of the maximum binding is achieved.
What is the volume occupied by 26.9g of argon gas at a pressure of 1.23 and a temperature of 374?
To calculate the volume of the gas, you would need the ideal gas law equation: PV = nRT. First, convert grams of argon to moles using the molar mass of argon. Then, plug the values of pressure (P), temperature (T), and gas constant (R) into the equation with the calculated number of moles (n) to solve for volume (V).
What is the volume occupied by 10.0 g of argon gas at a pressure of 1.12 ATM and a temperature of 307 K?
To calculate the volume of a gas, you can use the ideal gas law: (V = \frac{nRT}{P}), where (n) is the number of moles of the gas, (R) is the ideal gas constant, (T) is the temperature in Kelvin, and (P) is the pressure. First, calculate the number of moles of argon using its molar mass. Then, plug the values into the ideal gas law to find the volume.
Did Malta become occupied by Germany during World War 2?
Malta was never occupied by German or Italian troops, though it was under constant attscks from 1940 to 1943.
How do you calculate hotel occupancy in percentage?
Number of rooms occupied divided by total rooms in hotel times 100 For example if there are 50 rooms occupied and 200 rooms in the hotel, then 50/200 x 100 = 25% occupied
How do hotels calculate their Rack Rate and What is the formula?
Room revnue divided by total no. Of room occupied
