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$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$
Which statement about the above equation is wrong?
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The transition temperature for $\alpha$ to $\beta$ phase change is $600 \mathrm{~K}$ and $C_{p, \beta}-C_{p, \alpha}=1 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$. Assume $\left(C_{p, \beta}-C_{p, \alpha}\right)$ is independent of temperature in the range of 200 to $700 \mathrm{~K} . \mathrm{C}_{p, \alpha}$ and $C_{p, \beta}$ are heat capacities of $\alpha$ and $\beta$ phases, respectively.
($1$)The value of entropy change, $\mathrm{S}_\beta-\mathrm{S}_\alpha$ (in $\mathrm{J} \mathrm{mol}^{-1} \mathrm{~K}^{-1}$ ), at $300 \mathrm{~K}$ is. . . . . . .
[Use : $\ln 2=0.69$ Given : $S_\beta-S_\alpha=0$ at $\left.0 \mathrm{~K}\right]$
($2$) The value of enthalpy change, $\mathrm{H}_\beta-\mathrm{H}_\alpha$ (in $J$ mol ${ }^{-1}$ ), at $300 \mathrm{~K}$ is
Give the answer quetion ($1$) and ($2$)