Step 1: Write the system of equations clearly: \[ x + 3y + 7 = 0 \quad \text{(1)}, \] \[ 3x + 10y - 3z + 18 = 0 \quad \text{(2)}, \] \[ 3y - 9z + 2 = 0 \quad \text{(3)}. \] We will solve this system step by step.
Step 2: From equation (1), solve for \( x \): \[ x = -3y - 7 \quad \text{(4)}. \] Substitute equation (4) into equations (2) and (3) to simplify the system. \bigskip Step 3: Substituting \( x = -3y - 7 \) into equation (2): \[ 3(-3y - 7) + 10y - 3z + 18 = 0, \] \[ -9y - 21 + 10y - 3z + 18 = 0, \] \[ y - 3z - 3 = 0 \quad \text{(5)}. \] Now substitute equation (5) into equation (3).
Step 4: Substituting into equation (3): \[ 3y - 9z + 2 = 0, \] \[ y - 3z = -\frac{2}{3} \quad \text{(6)}. \] Now subtract equation (5) from equation (6): \[ 0 = 3 \quad \text{which is a contradiction.} \]
Step 5: Since we encounter a contradiction, the system of equations has no solution.
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.