Consider the reaction: 2NO(g) + 0₂ (8) - 2 NO₂ (g) Suppose that a particular moment during the reaction nitric oxide (NO) is reacting at a rate of -0.054 M S

The gas-phase decomposition of NOBr has a k= 0.82 M¹ s1 at 10°C. NOBr(g) → NO(g) + ½ Br₂ (g) rate k[ NOBr]² We start with 0.074 M NOBr in a flask at 10°C. 17T A. How long (in secs) does it take to use up 0.011 M of this NOBr? Only enter the number with no units 2.4

For a heterogeneous chemical system undergoing the reaction shown by the chemical equation below, which is never important to the rate of the forward reaction? (Hint: what does not affect the rate of the forward reaction) A (s)  +  B (g)  à  C (s)         temperatur of the system     pressure of gas B     surface area of solid A     volume of solid C

Methane and water react to form carbon monoxide and hydrogen, like this: CH₂(g) + H₂O(g) → CO(g) + 3H₂(g) 2 Imagine 169. mmol of CH4 and 169. mmol of H₂O are added to an empty flask, and then answer the following questions. What is the rate of the forward reaction before any CH4 or H₂O has been added to the flask? What is the rate of the forward reaction just after the CH4 and H₂O has been added to the flask? What is the rate of the forward reaction at equilibrium? How much CH4 is in the flask at equilibrium? Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. O Greater than zero, and greater than the rate of the reverse reaction. Zero. Greater than zero, but less than the rate of the reverse…