Consider the combustion of methane in oxygen to produce CO2 and water:                           CH4(g) + O2(g) --> CO2(g) + H2O(g) When methane is being consumed at a rate of 0.65 M/s, what is the rate at which water is being produced?

The reaction between N2O5 and water$$N2​O5​(g)+H2​O(g)2HNO3​(g)is a source of nitric acid in the atmosphere. The reaction is first order in each reactant. Write the rate law for the reaction.

Consider a reaction: A + B C and the rate law expression: Rate = k [A]"[B]" %3D According to the rate law, rate of a reaction depends on which of the following? Concentration of reactants Concentration of products Temperature Nature of solvent

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…