use the ideal gas last pv=nrt n= same for each one and R=8.314 j/mol*k
This is the temperature at which an experiment begins.
When air is compressed at the same temperate and volume space, pressure will increase in accordance with Boyle's Law which states: PV/T (initial) = PV/T (final) where P is pressure, V is volume and T is temperature.
As the starting length of the muscle is increased the initial velocity increases then decreases.
Assuming the amount of gas remains constant, we can use the ideal gas law to calculate the final absolute pressure. The initial pressure (P1) is 200 kPa and the final volume (V2) is 250 cm3. The initial temperature (T1) is 40 degrees Celsius or 313.15 Kelvin, and the final temperature (T2) is 20 degrees Celsius or 293.15 Kelvin. Using the equation (P1 * V1) / T1 = (P2 * V2) / T2, we can solve for the final absolute pressure (P2), which is approximately 400 kPa.
The volume of air increases proportionally as it is heated, according to the formula: PV/T = P'V'/T' Where P, V, and T are initial values for pressure, volume and temperature in absolute terms and P',V',and T' are the final values with a constant pressure the equation becomes: V/T = V'/T' to solve for final volume the equation is: VT'/T = V' if V=1cu. meter, T = 200K and T' = 300K then 1 cu.meter x 300K/200K = 1.5 cu.meter
BOYLES LAW The relationship between volume and pressure. Remember that the law assumes the temperature to be constant. or V1 = original volume V2 = new volume P1 = original pressure P2 = new pressure CHARLES LAW The relationship between temperature and volume. Remember that the law assumes that the pressure remains constant. V1 = original volume T1 = original absolute temperature V2 = new volume T2 = new absolute temperature P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature IDEAL GAS LAW P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature Answer BOYLES LAW The relationship between volume and pressure. Remember that the law assumes the temperature to be constant. or V1 = original volume V2 = new volume P1 = original pressure P2 = new pressure CHARLES LAW The relationship between temperature and volume. Remember that the law assumes that the pressure remains constant. V1 = original volume T1 = original absolute temperature V2 = new volume T2 = new absolute temperature P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature IDEAL GAS LAW P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature
The relationship between temperature and pressure is not named after a specific person, like Boyle's or Charles' Laws, but states that the relationship between the temperature and pressure of a gas (usually as observed in a rigid container) is direct. Therefore, as temperature increases, pressure does too.This is Gay-Lussac's law.The temperature and pressure of gasses are related. As the pressure increases the temperature also increases, and vice verse. As the pressure decreases the temperature gets colder.The ideal-gas law may be expressed as PV=nRT.Absolute temperature TNumber of moles (a measure of the number of molecules) nVolume VPressure PRydberg's constant R (some value that makes the numbers and the units work)Obviously, from the equation, you could half the temperature and keep the pressure the same, if, for example, you cut the volume in half. Or you could half the temperature and double the number of moles, and the pressure wouldn't change.
If pressure is held constant, volume and temperature are directly proportional. That is, as long as pressure is constant, if volume goes up so does temperature, if temperature goes down so does volume. This follows the model V1/T1=V2/T2, with V1 as initial volume, T1 as initial temperature, V2 as final volume, and T2 as final temperature.
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You think probable to a Dewar container.
During the time water absorb heat from the atmosphere if the initial temperature was lower.
You can calculate pressure and temperature for a constant volume process using the combined gas law.
When hot metal is added into the water then the metal looses its energy into the water and this heat is gained by the water, so the temperature gets increases when hot metal added into it i.e final temperature is greater than initial temperature of water.
You subtract the initial from the after, and the result is the change. If the initial temperature is 50º and the after is 70º, then the change is +20º.
Pressure has no effect on the mass of a given sample of gas. Whatever the initial mass is, it won't change, regardless of the pressure, unless you let more gas in or let some escape.
A: As power is turn on the temperature of the IC is at ambient temperature or the initial temperature then becomes the increase in temperature due to heating.
This cannot be answered without an initial volume or pressure. But the final pressure of an expansion of a gas can be determined by the following formula. PV/T = P'V'/T' where P = pressure absolute V = volume T = temperature absolute ( ' ) indicates the new pressure, volume and temperature because the temperature is constant this can be reduced to PV = P'V' or P' = PV/V'