A toxic gas is accidentally released into a sealed laboratory. The initial pressure of the gas is .05 atm but the level for safe exposure is 0.001 atm. The rate constant for first-order decomposition of this substance is known to be is 5.2 × 10–3 s-1.   How long (in s) will it take for the reactant to decompose enough for the area to be safe?

The reaction, A → products, is known to be second order with respect to the concentration of A and second order overall. The rate constant for the reaction is 0.0500 M-1·min-1 at a certain temperature.If the initial concentration of A is 0.650 M. What will the concentration of A be after 40.0 min?How long would it take for 45.0% of the starting material (A) to undergo reaction?

The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N2O5 → 4NO2 + O2 The rate constant at a given temperature is found to be 5.25 x 10-4 s-1. If the initial concentration of N2O5 is 0.11 M, what is its concentration after exactly 11 minutes have passed?   Round your answer to 2 decimal places.

If a catalyst was added to this reaction, would it change, not change, increase or decrease the overall order of this reaction

Butadiene (C4H6C4H6) reacts with itself to form a dimer with the formula (C8H12C8H12). The reaction is second order in C4H6C4H6. If the rate constant at a particular temperature is 4.0×10−2M−1s−14.0×10−2M−1s−1 What is the half-life (in minutes) of this reaction when the initial C4H6C4H6 concentration is 2.30×10−2 MM ? Express your answer using two significant figures How many minutes does it take for the concentration of C4H6C4H6 to drop from 1.20×10−2 MM to 6.00×10−3 MM ? Express your answer using two significant figures.

After 48 seconds, 10.% of reactant has reacted. If the reaction is a 1st order reaction, the special rate constant k = _.

The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) → ½ H2 (g) + ½ I2 (g) is zero order in HI with a rate constant of 1.20×10-4 M/s How much time is required for the concentration of HI to drop to 9.40×10-2 M if its initial concentration is 0.525 M?

A particular reactant decomposes with a half‑life of 117 s117 s when its initial concentration is 0.376 M.0.376 M. The same reactant decomposes with a half‑life of 221 s221 s when its initial concentration is 0.199 M.0.199 M. Determine the reaction order. 2 1 0   What is the value and units of the rate constant for this reaction? ?=k=     Units

The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N2O5 → 4NO2 + O2 The rate constant at a given temperature is found to be 5.25 x 10-4 s-1. If the initial concentration of N2O5 is 0.24 M, what is its concentration after exactly 9 minutes have passed?   Round your answer to 2 decimal places.

The decomposition of N,O, in solution in carbon tetrachloride is a first-order reaction. 2N,O, → 4NO2 + O2 The rate constant at a given temperature is found to be 5.25 x 104 s'. If the initial concentration of N,O5 is 0.16 M, what is its concentration after exactly 13 minutes have passed?