Flask is charged with 0.100 mol of A and allowed to react to form B according to
ID: 1004006 • Letter: F
Question
Flask is charged with 0.100 mol of A and allowed to react to form B according to the hypothetical gas-phase reaction A(g) B(g). The following data are collected: Calculate the number of moles of B at each time in the table, assuming that A is cleanly converted to B with no intermediates. Calculate the average rate of disappearance of A for each 40-s interval in units of mol/s. Which of the following would be needed to calculate the rate in units of concentration per time: the pressure of the gas at each time, the volume of the reaction flask, the temperature, or the molecular weight of A? Consider the following reaction: 2 NO(g) + 2 H2(g).N2(g) + 2 H2O(g) The rate law for this reaction is first order in H2 and second order in NO. Write the rate law. If the rate constant for this reaction at 1000 K is 6.0 * 10^4 M^2 s^-1, what is the reaction rate when [NO] - 0.035 M and [H2] - 0.01 M? What is the reaction rate at 1000 K w hen the concentration of NO is increased to 0.10 M, while the concentration of H2 is 0.010 M? What is the reaction rate at 1000 K if [NO] is decreased to 0.010 M and [H2] is increased to 0.030 M? For each of the following gas-phase reactions, write the rate expression in terms of the appearance of each product and disappearance of each reactant: 2 H2O(g) rightarrow 2 H2(g) + O2(g) 2 SO2(g) + O2(g) rightarrow 2 SO3(g) 2 NO(g) + 2 H2(g) rightarrow N2(g) + 2 H2O(g) N2(g) + 2 H2(g) rightarrow N2H4(g)Explanation / Answer
Answer-3)
For a general reaction,
aA + bB ----------------> cC + dD
Rate = -1/a(d[A]/dt = -1/b(d[B]/dt = 1/c (d[C]/dt) = 1/d(d[D]/dt).
Stoichiometric coefficients appear as reciprocals in rate expression.
-ve sign indicate decrease or disappearence of species as time progressess.
Using this,
a) 2H2O (g) ----------> 2H2 (g) + O2 (g).
Rate = -1/2 (d[H2O]/dt) = 1/2 (d[H2]/dt] = (d[O2]/dt).
b) 2SO2 (g) + O2 (g) -------------> 2SO3 (g)
Rate = - 1/2 (d[SO2]/dt) = - (d[O2]/dt] = 1/2 (d[SO3]/dt).
c) 2NO (g) + 2H2 (g) --------------> N2 (g) + 2H2O (g)
Rate = -1/2 (d[NO]/dt) = - 1/2 (d[H2]/dt] = (d[N2]/dt) = Rate = 1/2 (d[H2O]/dt).
d) N2 (g) + 2H2 (g) ----------> N2H4 (g)
Rate = - (d[N2]/dt) = - 1/2 (d[H2]/dt] = (d[N2H4]/dt).
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