Question

Suppose the decomposition of nitryl chloride proceeds by the following mechanism: step elementary reaction rate constant 1 NO?Cl(g) ? NO?(g) + Cl(g) k? 2 Cl(g) + NO?Cl(g) ? NO?(g) + Cl?(g) k? Suppose also $k_1 \gg k_2$. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observables rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of $k_1$, $k_2$, and (if necessary) the rate constants $k_{-1}$ and $k_{-2}$ for the reverse of the two elementary reactions in the mechanism. k = For each chemical reaction listed in the table below, decide whether the highlighted atom is being oxidized or reduced. reaction highlighted atom is being... either oxidized reduced oxidized nor reduced Na?CO?(s) + H?PO?(aq) ? Na?HPO?(aq) + CO?(g) + H?O(l) 4 HF(g) + SiO?(s) ? SiF?(g) + 2 H?O(g) N?(g) + 3 H?(g) ? 2 NH?(g) 4 KI(aq) + 2 CuCl?(aq) ? 2 CuI(s) + I?(aq) + 4 KCl(aq)

          Suppose the decomposition of nitryl chloride proceeds by the following mechanism:
step elementary reaction rate constant
1 NO?Cl(g) ? NO?(g) + Cl(g) k?
2 Cl(g) + NO?Cl(g) ? NO?(g) + Cl?(g) k?
Suppose also $k_1 \gg k_2$. That is, the first step is much faster than the second.
Write the balanced
chemical equation for the
overall chemical reaction:
Write the experimentally-
observables rate law for the
overall chemical reaction.
rate = k
Note: your answer should
not contain the
concentrations of any
intermediates.
Express the rate constant
k for the overall chemical
reaction in terms of $k_1$, $k_2$,
and (if necessary) the rate
constants $k_{-1}$ and $k_{-2}$ for
the reverse of the two
elementary reactions in
the mechanism.
k = 
For each chemical reaction listed in the table below, decide whether the highlighted atom is being oxidized or reduced.
reaction highlighted atom is being...
either
oxidized reduced oxidized nor
reduced
Na?CO?(s) + H?PO?(aq) ? Na?HPO?(aq) + CO?(g) + H?O(l)
4 HF(g) + SiO?(s) ? SiF?(g) + 2 H?O(g)
N?(g) + 3 H?(g) ? 2 NH?(g)
4 KI(aq) + 2 CuCl?(aq) ? 2 CuI(s) + I?(aq) + 4 KCl(aq)

Suppose the decomposition of nitryl chloride proceeds by the following mechanism:
step elementary reaction rate constant
1 NO?Cl(g) ? NO?(g) + Cl(g) k?
2 Cl(g) + NO?Cl(g) ? NO?(g) + Cl?(g) k?
Suppose also k1 ≫ k2. That is, the first step is much faster than the second.
Write the balanced
chemical equation for the
overall chemical reaction:
Write the experimentally-
observables rate law for the
overall chemical reaction.
rate = k
Note: your answer should
not contain the
concentrations of any
intermediates.
Express the rate constant
k for the overall chemical
reaction in terms of k1, k2,
and (if necessary) the rate
constants k-1 and k-2 for
the reverse of the two
elementary reactions in
the mechanism.
k =
For each chemical reaction listed in the table below, decide whether the highlighted atom is being oxidized or reduced.
reaction highlighted atom is being...
either
oxidized reduced oxidized nor
reduced
Na?CO?(s) + H?PO?(aq) ? Na?HPO?(aq) + CO?(g) + H?O(l)
4 HF(g) + SiO?(s) ? SiF?(g) + 2 H?O(g)
N?(g) + 3 H?(g) ? 2 NH?(g)
4 KI(aq) + 2 CuCl?(aq) ? 2 CuI(s) + I?(aq) + 4 KCl(aq)

Added by Catherine C.

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