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Which is a correct description of the partial pressures of N2O4 and NO2?

Correct Answer: The partial pressure of NO2 is increasing twice as fast as that of N2O4 is decreasing.
(D) When the reaction occurs, the N2O4 must decrease and the NO2 must increase. (D) is the only response that expresses this fact.

If u (x, y, z, t) = f(x + iβy - vt) + g(x - iβy - vt), where f and g are arbitrary and twice differentiable functions, is a solution of the wave equation $$\frac{{\partial {u^2}}}{{\partial {x^2}}} = \frac{{{\partial ^2}u}}{{\partial {y^2}}} = \frac{1}{{{c^2}}}\frac{{{\partial ^2}u}}{{\partial {t^2}}}$$     then β is

The dimerization of NO2(g) to N2O4(g) is an endothermic process. Which of the following will, according to Le Châtelier's principle, increase the amount of N2O4 in a reaction vessel?

50°C তাপমাত্রায় N2O4 বিয়োজনের KP এর মান 3.11 atm । সাম্যমিশ্রনে NO2 এর আংশিক চাপ 0.45 atm হলে N2O4 এর আংশিক চাপ কত?

298K তাপমাত্রায় সাম্যবস্থায় N2O4 এর বিয়োজন মিশ্রণে N2O4 এর আংশিক চাপ 0.8 atm এবং বিক্রিয়াটির Kp= 0.008 atm। NO2 এর আংশিক চাপ নির্ণয় কর।

According to Dalton's law of partial pressures, (where pb = Barometric pressure, pa = Partial pressure of dry air and pv = Partial pressure of water vapour)

Let $${\text{f}}\left( {{\text{x, y}}} \right) = \frac{{{\text{a}}{{\text{x}}^2} + {\text{b}}{{\text{y}}^2}}}{{{\text{xy}}}},$$     where a and b are constants. If $$\frac{{\partial {\text{f}}}}{{\partial {\text{x}}}} = \frac{{\partial {\text{f}}}}{{\partial {\text{y}}}}$$   at x = 1 and y = 2, then the relation between a and b is

The equation relating E, P, V and T which is true for all substanes under all conditions is given by $${\left( {\frac{{\partial {\text{E}}}}{{\partial {\text{V}}}}} \right)_{\text{T}}} = {\text{T}} \cdot {\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{T}}}}} \right)_{\text{H}}} - {\text{P}}{\text{.}}$$      This equation is called the

The highest pressure gas of a mixture has partial pressure p, the partial pressure of other gases decreases by factor of 2n-1, the partial pressure of second gases decreases by a factor of 2, partial pressure of third gas increases by 4, and so on, if the total pressure of gas mixture is 31p/16, how many gases are present in the mixture?

On a P-V diagram of an ideal gas, suppose a reversible adiabatic line intersects a reversible isothermal line at point A. Then at a point A, the slope of the reversible adiabatic line $${\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)_{\text{S}}}$$  and the slope of the reversible isothermal line $${\left( {\frac{{\partial {\text{P}}}}{{\partial {\text{V}}}}} \right)_{\text{T}}}$$  are related as (where, $${\text{y}} = \frac{{{{\text{C}}_{\text{p}}}}}{{{{\text{C}}_{\text{v}}}}}$$  )

Maxwell equation $${\left( {\frac{{\partial P}}{{\partial T}}} \right)_V} = {\left( {\frac{{\partial S}}{{\partial V}}} \right)_T}$$     is produced from which of the following equation