Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0080 M.s¹: 2 NH3(g) → N₂ (g) + 3H2(g) Suppose a 250. mL flask is charged under these conditions with 100. mmol of ammonia. How much is left 10. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. X x10

A reaction proceeds according to the following equation:                              A + 3B → 2C + 2D At an early stage of the reaction, conc. A = 1.191 M and 6.06 minutes later, conc. A= 0.949 M.  What is the average rate of the reaction during this time period, expressed in units of M·s-1?

Consider the reaction : 3A + 2B →  4C Initially, and at some fixed temperature, the reaction proceeds at such a rate that 2.3 millimoles of A are consumed in 1 minute and 12 secondes. The reaction takes place in 1 L. The following table contains the experimental data for the reaction. (Taken from Ball. Physical Chemistry, 2nd edition, 2006) Rate (M/s) [A], M [B], M 1.081 x 10-5 0.660 1.23 6.577 x 10-5 4.01 1.23 6.568 x 10-5 4.01 2.25   c. Determine the partial order on A. Partial order on B is 0. d. What is the order of the reaction.

Measuring total pressure is a convenient way to monitor gas reaction: 2NOCl(g) → 2NO(g) + Cl2(g). The rate of the reaction depends on the concentration of the reactant, which is proportional to the partial pressure of the reactant. Derive a relation connecting its velocity above reaction with initial pressure, P0, and total pressure, Pt, at time t.(Hint: Assume the reaction is 2nd order. Make a table with initial (t0) and final values ​​(t) of the moles of NOCl, NO, and Cl2, and construct the ideal gas equations for both cases. Use the ideal gas equation for t0 so that calculate the initial concentration of NOCl and substitute this value into the equation of ideal gases for t)