what pressure would you expect if the gas in the flask were heated to 150 degrees celsius?
insufficient information,cant ans it
What was the initial temperature? Is the gas sealed inside the flask?
To determine the pressure of the gas in the flask when it is heated to 150 degrees Celsius, we can use the ideal gas law, which relates pressure, volume, temperature, and the number of moles of the gas.
The ideal gas law is expressed as:
PV = nRT
where:
P is the pressure of the gas (in units of pressure, such as atmospheres or pascals)
V is the volume of the gas (in units of volume, such as liters)
n is the number of moles of the gas
R is the ideal gas constant (in units that depend on the units of pressure, volume, and temperature)
T is the temperature of the gas (in units of temperature, such as Kelvin)
To use the ideal gas law, we need to convert the temperature from degrees Celsius to Kelvin. This can be done by adding 273.15 to the temperature in degrees Celsius. In this case, we have:
T = 150 °C + 273.15 = 423.15 K
Now, if we assume that the volume, number of moles, and gas constant remain constant, we can rearrange the ideal gas law to solve for pressure:
P = nRT / V
Given that the volume, number of moles, and gas constant are constant, the equation simplifies to:
P = kT
where k is a constant.
Plugging in the values, we have:
P = k * 423.15 K
Without knowing the specific gas constant or other details, we can conclude that the pressure of the gas in the flask would increase when it is heated to 150 degrees Celsius. However, we cannot determine the exact value of the pressure without additional information.