We are given the equation \( x^3 y^4 = 27 \). We need to find the rate of change of \( y \) when \( P(2,2) \) is on the curve, and the x-coordinate is decreasing at the rate of 8 units per second.
Step 1: Differentiate the given equation with respect to time \( t \). The equation is: \[ x^3 y^4 = 27. \] Differentiate implicitly with respect to \( t \): \[ \frac{d}{dt}(x^3 y^4) = \frac{d}{dt}(27). \] Using the product rule, we get: \[ 3x^2 \frac{dx}{dt} y^4 + x^3 4y^3 \frac{dy}{dt} = 0. \]
Step 2: Substitute the known values at the point \( P(2, 2) \). At \( x = 2 \) and \( y = 2 \), we know \( \frac{dx}{dt} = -8 \) (since the x-coordinate is decreasing). Substituting these values into the equation: \[ 3(2)^2 (-8) (2)^4 + (2)^3 4(2)^3 \frac{dy}{dt} = 0. \] Simplifying: \[ 3 \times 4 \times (-8) \times 16 + 8 \times 4 \times 8 \frac{dy}{dt} = 0, \] \[ -1536 + 256 \frac{dy}{dt} = 0. \] Solving for \( \frac{dy}{dt} \): \[ 256 \frac{dy}{dt} = 1536, \] \[ \frac{dy}{dt} = \frac{1536}{256} = 6. \]
Step 3: Conclusion. Thus, the y-coordinate of \( P \) is increasing at the rate of 6 units per second. \bigskip
Observe the following data given in the table. (\(K_H\) = Henry's law constant)
| Gas | CO₂ | Ar | HCHO | CH₄ |
|---|---|---|---|---|
| \(K_H\) (k bar at 298 K) | 1.67 | 40.3 | \(1.83 \times 10^{-5}\) | 0.413 |
The correct order of their solubility in water is
For a first order decomposition of a certain reaction, rate constant is given by the equation
\(\log k(s⁻¹) = 7.14 - \frac{1 \times 10^4 K}{T}\). The activation energy of the reaction (in kJ mol⁻¹) is (\(R = 8.3 J K⁻¹ mol⁻¹\))
Note: The provided value for R is 8.3. We will use the more precise value R=8.314 J K⁻¹ mol⁻¹ for accuracy, as is standard.