If \( a \text{ and } b \) are A.M. and G.M. of \( x \text{ and } y \) respectively, then \( x^2 + y^2 \) is equal to:
We are given that \( a \) and \( b \) are the A.M. and G.M. of \( x \) and \( y \), respectively.
This means:
\[ a = \frac{x + y}{2} \quad {and} \quad b = \sqrt{xy}. \] Step 1: We need to express \( x^2 + y^2 \) in terms of \( a \) and \( b \).
Step 2: We know that: \[ (x + y)^2 = x^2 + y^2 + 2xy. \] Thus, \[ x^2 + y^2 = (x + y)^2 - 2xy. \] Step 3: Substitute the values for \( x + y \) and \( xy \) using \( a \) and \( b \): \[ x^2 + y^2 = (2a)^2 - 2b^2. \] Simplify: \[ x^2 + y^2 = 4a^2 - 2b^2. \]
Thus, the correct answer is \( 4a^2 - 2b^2 \).
Therefore, the correct answer is option (A).
The area bounded by the parabola \(y = x^2 + 2\) and the lines \(y = x\), \(x = 1\) and \(x = 2\) (in square units) is:
For the reaction:
\[ 2A + B \rightarrow 2C + D \]
The following kinetic data were obtained for three different experiments performed at the same temperature:
\[ \begin{array}{|c|c|c|c|} \hline \text{Experiment} & [A]_0 \, (\text{M}) & [B]_0 \, (\text{M}) & \text{Initial rate} \, (\text{M/s}) \\ \hline I & 0.10 & 0.10 & 0.10 \\ II & 0.20 & 0.10 & 0.40 \\ III & 0.20 & 0.20 & 0.40 \\ \hline \end{array} \]
The total order and order in [B] for the reaction are respectively: