For the following reaction\(2 \mathbf{X}+\mathbf{Y} \stackrel{k}{\rightarrow} \mathbf{P}\)the ra.... VIDEO
For the following reaction\(2 \mathbf{X}+\mathbf{Y} \stackrel{k}{\rightarrow} \mathbf{P}\)the rate of reaction is \(\frac{d[\mathrm{P}]}{d t}=k[\mathbf{X}]\). Two moles of \(\mathbf{X}\) are mixed with one mole of \(\mathbf{Y}\) to make \(1.0 \mathrm{~L}\) of solution. At \(50 \mathrm{~s}, 0.5 \mathrm{~mole}\) of \(\mathbf{Y}\) is left in the reaction mixture. The correct statement(s) about the reaction is(are)(Use: \(\ln 2=0.693\) ) 📲PW App Link - https://bit.ly/YTAI_PWAP 🌐PW Website - https://www.pw.live
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