SO_{2}Cl_{2} rightarrow SO_{2}+Cl_{2} is a first order gas reaction with k=2.2times 10^{-5}sec^{-1} 320^o C. The percentage of SO_{2}Cl_{2} decomposed on heating 90 minutes is:1.1180.111818.1111.18 (2024)
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SO2Cl2→SO2+Cl2 is a first order gas reaction with k=2.2×10−5sec−1 at 320oC. The percentage of SO2Cl2 decomposed on heating for 90 minutes is:
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SO2Cl2(g)→SO2(g)
The given reaction is a first order gas reaction with k=2.2×10−5sec−1 at 320∘C. What % of SO2Cl2 is decomposed on heating this gas for 90 min?
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The reaction SO2Cl2→SO2+Cl2, is a first order gas reaction with k=2.2×10−5s−1 at 573K. What percent of SO2Cl2 is decomposed on heating at 573K for 90min?
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Time required to decompose SO2CL2 to half of its initial amount is 60 minutes . If the decompose is a first order reaction, calculate the rate constant of the reaction.
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Timerequired to decompose SO2Cl2to half of its initial amount is 60 minutes. If the decomposition isa first order reaction, calculate the rate constant of the reaction.
Answer: The reaction SO₂Cl₂(g)→SO₂(g)+Cl2(g) is a first-order reaction with a half-life of 3.15 ×10⁴s at 320°C. Then 11.2% of SO₂Cl₂ would be decomposed on heating at 320°C for 90 min. here [A₀] denotes the concentration of SO₂Cl₂ at t=0.
The reaction SO2Cl2(g) → SO2(g) + Cl2(g) is first order with a rate constant of 2.2 x 10^(-5) s^(-1) at 320°C. What fraction of a sample of SO2Cl2 will remain if it is heated for 5.0 hr at 320°C? A drink that contains 4 1/2 ounces of a proof liquor… approximately how many drinks does this beverage contain?
t=3 hr. The half-life period of a first order reaction is 1 hr. What is the time in hour taken for 87.5% completion of the reaction? The time for half life of a first order reaction is 1 HR.
If the initial concentration of the reactants is increased, the half life period for a first order reaction remains unchanged. This is because the half life period for a first order reaction is independent of the initial concentration.
Sulfuryl chloride reacts with water, releasing hydrogen chloride gas and sulfuric acid: 2 H2O + SO2Cl2 → 2 HCl + H2SO. For sulfuryl chloride, this happens at room temperature, but the related sulfuryl fluoride does not hydrolyse at temperatures up to 150 °C.
(a) The gas-phase decomposition of SO2Cl2, SO2Cl21g2 ¡SO21g2 + Cl21g2, is first order in SO2Cl2. At 600 K the half-life for this process is 2.3 * 105 s.
As described in Exercise 14.41, the decomposition of sulfuryl chloride 1SO2Cl22 is a first-order process. The rate constant for the decomposition at 660 K is 4.5 * 10-2 s-1.
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