Oxidation, reduction and redox agents

The second step converts nitrogen monoxide to nitrogen dioxide. $\ce{2NO(g) + O2(g) <=> 2NO2(g)}$ $\Delta H^\ominus = -114\ \mathrm{kJ\,mol^{-1}}$ (i) Identify the oxidation state of nitrogen in $\ce{NO}$ and in $\ce{NO2}$. (ii) State the equilibrium constant…

Which statement about this reaction is correct? $\ce{2Cl2 + O2 -> 2Cl2O}$ A. Chlorine is the reducing agent. B. Oxygen is the reducing agent. C. Chlorine is reduced. D. Oxygen is oxidized.

A related nitrile, ethanenitrile, $\ce{CH3CN}$, reacts with hydrogen according to the equilibrium: $\ce{CH3CN(g) + 2H2(g) <=> CH3CH2NH2(g)}$ (i) Write the expression for the equilibrium constant, $K$, for this reaction. (ii) Determine the oxidation states that…

Nitrogen dioxide reacts with rain water and oxygen to form nitric acid. (i) State an equation for this reaction, including state symbols. (ii) Explain, with reference to the oxidation states of two elements, why this is a redox reaction. (iii) Describe the…

Which change represents oxidation of the functional group? A. $\ce{CH3COCH3 -> CH3CH(OH)CH3}$ B. $\ce{CH3CH(OH)CH3 -> CH3COCH3}$ C. $\ce{CH3CH2COOH -> CH3CH2CHO}$ D. $\ce{CH3CH=CH2 -> CH3CH2CH3}$

Sulfur dioxide can also be removed from flue gas by reaction with hydrogen peroxide, forming sulfuric acid. $\ce{SO2(g) + H2O2(aq) -> H2SO4(aq)}$ Deduce which element is reduced in this process, indicating the initial and final oxidation states. Element…

Deduce the oxidation state of bromine in the reactant and in each of the two products. Reactant $\ce{Br2}$: Product $\ce{HOBr}$: Product $\ce{HBr}$:

Calcium hydride is used as a portable source of hydrogen for fuel cells. It reacts with water as shown. $\ce{CaH2(s) + 2H2O(l) -> Ca(OH)2(aq) + 2H2(g)}$ Which statement is correct? A. Calcium is reduced from +2 to 0. B. Hydrogen in $\ce{CaH2}$ is oxidized from…