Sulfuryl chloride, , decomposes when heated. In an experiment, the initial concentration of sulfuryl chloride was 2.11*10^-2 mol/L. If the rate constant is 2.2*1-^-5 /s, what is the concentration of sulfuryl chloride after 3.0 hr? The reaction is first order.
For the first order reaction
Since the rate constant is given in terms of s^(-1), we need to convert the time of 3.0 hours by multiplying it with 3600
Note - Post any doubts/queries in comments section.
Sulfuryl chloride, , decomposes when heated. In an experiment, the initial concentration of sulfuryl chloride was...
At a fixed temperature, Sulfuryl chloride, SO2Cl2 gas decomposes to sulfur dioxide and chlorine gas in a first-order reaction, with the rate constant of 2.90 x 10-4 s-1. SO2Cl2 (g ) ⟶ SO2 (g) + Cl2 (g) 1.) If the initial C4H8 concentration is 0.225 M, what is the concentration after 900 s? 2.) Use the value of k to calculate the half-life of SO2Cl2 (g) in seconds. its SO2Cl not C4H8
10 and 11
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1a. Hydrogen iodide decomposes when heated, forming H2 (g) and I2 (g). The rate law for this reaction is -delta[HI]/delta t = k[HI]^2. At 443 °C, k=30.L/molxmin. If the initial HI (g) concentration is 5.5x10^-2 mol/L, what concentration of HI (g) will remain after 10. minutes? Concentration = ____ mol/L 1b. The decomposition of SO2Cl2 SO2Cl2 (g) ----> SO2 (g) + Cl2 (g) is first-order in SO2Cl2, and the reaction has a half-life of 245 minutes at 600 K. If...
Sulfuryl chloride (SO2Cl2) decomposes into sulfur dioxide (SO2) and chlorine (C12) according to the following chemical equation. SO2C12(g) → SO2(g) + C12() The half-life for the decomposition of sulfuryl chloride at 320 °C is 8.75 h, regardless of its initial concentration. A rigid vessel initially contains only SO2C12(g) at a pressure of 722 mmHg. What is the total pressure in the reactor, measured at 320 °C, 3.00 h after the start of the reaction? ANS: 875 mmHg
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