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When a sample of gas is compressed from 6.0 L to 2.0 L at a constant temperature the pressure of the gas doubles?
Are you stating or asking ? If that's a statement, then it's an incorrect one. At constant temperature, the product of (pressure) x (volume) is constant. So, if the volume changed by a factor of 3, the pressure must also change by a factor of 3 ... the pressure must triple.
When a sample of gas is compressed from 6.0 L to 2.0 L at a constant temperature the pressure of the gas doubles.?
Are you stating or asking ? If that's a statement, then it's an incorrect one. At constant temperature, the product of (pressure) x (volume) is constant. So, if the volume changed by a factor of 3, the pressure must also change by a factor of 3 ... the pressure must triple.
What does nine fifths have to do with the Celsius and Fahrenheit scale?
Celsius and fahrenheita re f diffrent scales. 1 degree C =9/5 F. So 100 C change is 9/5 (100) = 180F change But since the C scale is 0 at frex=zing water and F scale is 32 at freezing water, then F = 9/5C + 32
If you want to predict how temperature will affect the volume of a gas what other factor must be held constant?
pressure
Does an increase in pressure at constant temperature increase the rate constant of a reversible reaction in both directions?
The rate constant is unaffected, as demonstrated by Arrhenius equation: k = Ae^(-E/RT) where A is the pre-exponential factor (constant for a particular reaction) E is the activation energy R is the molar gas constant T is the thermodynamic temperature However, when pressure is increased at constant temperature for a gaseous reversible reaction, the concentrations of every reactant and product increase by the SAME factor. Since Kp (pressure equilibrium constant) is to remain constant, it means that the position of equilibrium will shift in such a way so as to decrease the total number of moles of gaseous species. Note: This answer can be improved by proving the last statement using a general example which, due to lack of time, I skipped. (Although some people might get the logic!!!)
Factor that can change equilibrium constant?
Temperature
How do you write the conversion factor for Celsius and Kelvin?
Celsius to Kelvin conversion formula The temperature T in Kelvin (K) is equal to the temperature T in degrees Celsius (°C) plus 273.15: T(K) = T(°C) + 273.15
What is a constant factor in an experiment?
The factor that doesnt change in your experiment
What is a factor that cannot be changed during a experiment?
A constant factor is one maintained unchanged throughout an experiment so that it does not affect the outcome. These are also referred to as controlled variables.
The factor that does not change in an experiment is the?
The factor that does not change in an experiment is called the control variable or constant. It is used as a baseline for comparison against the variables that are being tested to determine their effect.
When using Charles law the units of temperature can be either Kelvin or degree Celsius?
Yes, that is correct. Charles's Law states that the volume of a gas is directly proportional to its temperature, assuming pressure and amount of gas are constant. The temperature can be measured in Kelvin or degrees Celsius because they both have the same unit size and are related by a simple conversion factor (Kelvin = Celsius + 273.15).
What is a constant factor used in an experiment?
The factor that doesnt change in your experiment
Does doubling celsius temperature double pressure?
Using the Celsius temperature scale, it is not correct. But doubling the temperature using the Kelvin temperature scale, where zero is the absolute minimum gegree possible, will double pressure . p1/T1=p2/T2=constant.
A factor that does not change in an experiment?
Controlled variable.
What is the conversion factor between imperial temperature units and metric temperature units?
The conversion factor between imperial temperature units (Fahrenheit) and metric temperature units (Celsius) is 5/9.
When a sample of gas is compressed from 6.0 L to 2.0 L at a constant temperature the pressure of the gas doubles.?
Are you stating or asking ? If that's a statement, then it's an incorrect one. At constant temperature, the product of (pressure) x (volume) is constant. So, if the volume changed by a factor of 3, the pressure must also change by a factor of 3 ... the pressure must triple.
When a sample of gas is compressed from 6.0 L to 2.0 L at a constant temperature the pressure of the gas double?
Are you stating or asking ? If that's a statement, then it's an incorrect one. At constant temperature, the product of (pressure) x (volume) is constant. So, if the volume changed by a factor of 3, the pressure must also change by a factor of 3 ... the pressure must triple.
