The specific heat of gases can be taken roughly as a constant for differences in the order of 100⁰ C from ambient. Variation is crucial and cannot be disregarded for temperatures of more than, let's say 500 ⁰C or 1000⁰C.
- The ideal gas constant is the difference between cp and cv for low pressures (the ideal gas).
- The classical statistical physics principles for ideal non-interacting gases are found in any university physics primer.
- The demonstration that pV/T = constant is typically included in texts on macroscopic thermodynamics suggests that while temperature changes depend on specific heats, the opposite is also true.
- Real gas behavior requires a more complex explanation.
- As a result, we employ two techniques to determine the specific heat of gases: at constant volume and constant pressure.
- The value of the heat capacity at constant pressure is always greater than the value of the heat capacity at constant volume because the former also takes into account the value of the heat energy required to expand the substance against the constant pressure as its temperature rises.
To learn about Real gas
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PH of solution will be greater than seven (pH>7), that means that solution is basic (<span>pH above </span>7<span> is a base, the higher the number, the stronger is the base).
</span>pH (potential of hydrogenis) is a measure of the hydrogen ion (H⁺) concentration of a solution. <span>Solutions with a pH less than 7 are acidic.</span>
Susan should follow PEMDAS,
Parentheses
Exponents
Multiplication
Division
Addition
Subtraction,
So, the first step should be, to solve the equation in the parentheses.
I hope this helps!
