oxidation of iodide ion by H3AsO4 4.8×10^(-4) M/s

The oxidation of iodide ion by arsenic acid, H3AsO4,

is described by the balanced equation

3I^-(aq) + H3AsO4(aq) + 2H^+(aq)

→ I3^-(aq) + H3AsO3(aq) + H2O(l)

a) If –Δ[I^-]/Δt = 4.8×10^(-4) M/s,

what is the value of Δ[I3^-]/Δt

during the same time interval?

Express your answer using two significant figures.

b) What is the average rate of consumption

of H^+ during that time interval?

Express your answer using two significant figures.

비소산(H3AsO4)에 의한 아이오딘화 이온의 산화는

다음 균형 반응식으로 기술된다.

3I^-(aq) + H3AsO4(aq) + 2H^+(aq)

→ I3^-(aq) + H3AsO3(aq) + H2O(l)

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[참고] 평균 반응 속도

[참고] 반응 속도의 종류. 반응 속도식의 종류

a) If –Δ[I^-]/Δt = 4.8×10^(-4) M/s,

what is the value of Δ[I3^-]/Δt

during the same time interval?

–Δ[I^-]/Δt = 4.8×10^(-4) M/s

Δ[I^-]/Δt = –4.8×10^(-4) M/s

Δ[I3^-]/Δt = –(1/3) Δ[I^-]/Δt

= –(1/3) (–4.8×10^(-4) M/s)

= +1.6×10^(-4) M/s

---> (+)부호는

생성물인 I3^-의 생성 속도임을 의미.

답: 1.6×10^(-4) M/s

b) What is the average rate of consumption

of H^+ during that time interval?

–(1/2) (Δ[H^+]/Δt) = –(1/3) Δ[I^-]/Δt

Δ[H^+]/Δt = (2/3) Δ[I^-]/Δt

= (2/3) (–4.8×10^(-4) M/s)

= –3.2×10^(-4) M/s

---> (–)부호는

반응물인 H^+의 소모(소비) 속도임을 의미.

답: 3.2×10^(-4) M/s

[키워드] 평균 반응 속도 기준