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How is the dry gas pressure calculated when collecting gases over water?
The dry gas pressure when collecting gases over water is calculated by subtracting the vapor pressure of water at the given temperature from the total pressure of the gas collected.
According to Charless law whenever the temperature of a gas at constant pressure decreases the volume increases.true or false?
Answer: No, this is not according to Charles law; however according to Boyles law this statement is correct ('true').Charles' law states: When the pressure on a sample of a gas is held constant, the Kelvin temperature and the volume will be directly related.Boyle's law describes how the pressure of a gas tends to decrease as the volume of a gas increases when temperature is held constant.
What happens to the pressure of a confined gas at a constant temperature when the volume is reduced by half?
When the volume of a confined gas is reduced by half at a constant temperature, the pressure of the gas will double according to Boyle's Law. This is because the product of pressure and volume is constant for a given amount of gas at constant temperature. When the volume decreases, the pressure increases to maintain this equilibrium.
How can I use the collecting gas over water calculator to determine the amount of gas collected over water?
To use the collecting gas over water calculator to determine the amount of gas collected over water, you need to input the volume of gas collected and the temperature and pressure of the gas. The calculator will then calculate the amount of gas collected over water based on these inputs.
What does the pressure vs temperature graph reveal about the relationship between pressure and temperature in the system?
The pressure vs temperature graph shows that there is a direct relationship between pressure and temperature in the system. As temperature increases, pressure also increases, and vice versa. This relationship is known as the ideal gas law.
What is Charless Laws?
Charles' Law states that there is a direct mathematical relationship between volume and temperature of a gas.
If oxygen gas is collected over water at temperature of 10C and pressure of 1.02 ATM and the volume of gas plus water vapor collected is 293 mL then what volume of oxygen at STP was collected?
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What happens to volume when temperature of gas is decresd at constant pressure?
If the temperature of the gas is decreasing, then in order to maintain constant pressure, you would have to compress it in volume.
How is the temperature of CO2 determined if a thermometer is not present in the space in which the CO2 is collected?
If a thermometer is not present, you can estimate the temperature of CO2 by measuring the pressure inside the container where CO2 is collected. Using the ideal gas law, you can infer the temperature based on the pressure and volume of the gas. This assumes ideal gas behavior and neglects factors like non-ideal behavior or phase changes.
How is the dry gas pressure calculated when collecting gases over water?
The dry gas pressure when collecting gases over water is calculated by subtracting the vapor pressure of water at the given temperature from the total pressure of the gas collected.
As the temperature of a gas increases the volume of the gas must also increase to maintain constant pressure.?
That is correct. it's called Charles's law. it shows the connection between a gases temperature and its volume. in order to maintain constant pressure you must increase the volume of the container holding the gas if you increase the temperature of the gas.
Does temperature of a gas increase or decrease under pressure?
When pressure on a gas increases, its temperature also increases. This relationship is described by the ideal gas law (PV = nRT), showing that an increase in pressure leads to an increase in temperature to maintain the same volume and number of moles of gas.
According to Charless law whenever the temperature of a gas at constant pressure decreases the volume increases.true or false?
Answer: No, this is not according to Charles law; however according to Boyles law this statement is correct ('true').Charles' law states: When the pressure on a sample of a gas is held constant, the Kelvin temperature and the volume will be directly related.Boyle's law describes how the pressure of a gas tends to decrease as the volume of a gas increases when temperature is held constant.
What happens to the pressure of a confined gas at a constant temperature when the volume is reduced by half?
When the volume of a confined gas is reduced by half at a constant temperature, the pressure of the gas will double according to Boyle's Law. This is because the product of pressure and volume is constant for a given amount of gas at constant temperature. When the volume decreases, the pressure increases to maintain this equilibrium.
To maintain 40 degree evaporator coil temperature what is the suction pressure?
The suction pressure required to maintain a 40 degree evaporator coil temperature depends on the refrigerant being used, as different refrigerants have different pressure-temperature characteristics. A typical range for R-22 refrigerant would be around 55-60 psig. It is important to consult the specific pressure-temperature chart for the refrigerant being used.
If the volume and number of moles of gas are held constant as the temperature increase what will the pressure do?
If the volume and number of moles of gas are constant, then according to the ideal gas law, pressure is directly proportional to temperature. As temperature increases, the pressure will also increase in order to maintain equilibrium.
Is there any on board computer with microprocessor 8086 that use to measure temperature and pressure?
Yes, there are on-board computers with microprocessor 8086 that can be used to measure temperature and pressure. These computers can be equipped with sensors for temperature and pressure measurements, and programmed to process and display the data collected from these sensors in real-time. The 8086 microprocessor is capable of handling the data processing requirements for these measurements.
