For a chemical reaction 4 A+3 B→6C+9D rate of formation of C is 6×10−2 mol L−1 s−1 and rate of disappearance of A is 4×10−2 mol L−1 s−1. The rate of reaction and amount of B consumed in interval of 10 seconds, respectively will be:
Held on 30 Apr 2022 · Verified 9 Jul 2026.
1×10−2 mol L−1 s−1 and 30×10−2 mol L−1
10×10−2 mol L−1 s−1 and 10×10−2 mol L−1
1×10−2 mol L−1 s−1 and 10×10−2 mol L−1
10×10−2 mol L−1 s−1 and 30×10−2 mol L−1
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For the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g), ΔH = -198 kJ. Which condition favours forward reaction?
The unit of rate constant for a first-order reaction is:
For the reaction $\mathrm{A}(\mathrm{g}) \rightleftharpoons 2 \mathrm{~B}(\mathrm{~g})$, the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500 , at 1000 K . [Given : $\mathrm{R}=0.0831 \mathrm{~L} \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ ] $\mathrm{K}_{\mathrm{p}}$ for the reaction at 1000 K is
$\mathrm{C}(\mathrm{~s})+2 \mathrm{H}_2(\mathrm{~g}) \rightarrow \mathrm{CH}_4(\mathrm{~g}) ; \Delta \mathrm{H}=-74.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$ Which of the following diagrams gives an accurate representation of the above reaction? $[\mathrm{R} \rightarrow$ reactants; $\mathrm{P} \rightarrow$ products $]$
$\begin{aligned} &\text { Consider the following compounds: }\\ &\mathrm{\underline{K}O}_2, \mathrm{H}_2 \mathrm{\underline{O}}_2 \text { and } \mathrm{H}_2 \mathrm{\underline{S}O}_4 \text {. } \end{aligned}$ The oxidation states of the underlined elements in them are, respectively,
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