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6.75 g of SO2Cl2 was

A gaseous reaction mixture contains SO2, Cl2, and SO2Cl2 in a 2 L container with the gases having the following partial
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2. asked by Hannah
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1. The first order rate constant for the reaction, SO2Cl2(g) → SO2(g) + Cl2(g), is 2.20 x 10-5 s-1 at 593 K. What percent of a
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2. asked by renee
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Use the data in the table to determine how long it will take for half of the original amount of SO2Cl2 to decompose at the
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2. asked by Chloe
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The decomposition of SO2Cl2 is first order and has a rate constant of + 2.90 x 10^–4 s^–1. What is the concentration of
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2. asked by kayli
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Sulfuryl chloride, SO2Cl2, decomposes to SO2 and Cl2 according to the reactionSO2Cl2(g) -> SO2(g) + Cl2(g) The reaction is first
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2. asked by ssss
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6.75 g of SO2Cl2 was placed in a 2.00L flask. At 648 K 0.0345 moles of SO2 was present. Kc for the reaction SO2Cl2 <=> SO2 + Cl2
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2. asked by Ken
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At 100 °C the reaction:SO2Cl2(g) ⇄ SO2(g) + Cl2(g) has Kp = 2.4. Calculate the equilibrium composition of the mixture when
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2. asked by Anonymous
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The first-order reaction, SO2Cl2---> SO2 + Cl2, has a rate constant equal to 2.20 x 10^-5 s^-1 at 593 K. What percentage of the
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2. asked by hahaha
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The first-order reaction, SO2Cl2 �¨ SO2 + Cl2, has a rate constant equal to 2.20 �~ 10-5 s-1 at 593 K. What percentage of the
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2. asked by JOSEPH
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The first-order reaction, SO2Cl2 �¨ SO2 + Cl2, has a rate constant equal to 2.20 �~ 10-5 s-1 at 593 K. What percentage of the
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2. asked by JOSEPH
3. 1,265 views