Which statement concerning the reversible reaction 2 NO2(g) N2O4(g) is true? a. NO2 is the product of the...
- Which statement concerning the reversible reaction 2 NO2(g) N2O4(g) is true?
a. NO2 is the product of the forward reaction.
b. The reverse reaction produces N2O4.
c. At the start of the reaction, the forward and reverse reaction rates are equal.
d. As the forward reaction progresses and more N2O4 is formed, the reverse reaction rate
increases.
Homework Answers
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Which statement concerning the reversible reaction 2
NO2(g) N2O4(g) is true?
a. NO2 is the product of
the...
Which statement concerning the reversible reaction is true? 2 NO2(g) ↔ N2O4(g) A. At equilibrium an...
Which statement concerning the reversible reaction is true? 2 NO2(g) ↔ N2O4(g) A. At equilibrium an increase in Pressure will favor more N2O4 B. At the start of the reaction, the forward and reverse reaction rates are equal. C. NO2 is the product of the forward reaction. D. The reverse reaction produces N2O4
Give an example of a reversible reaction and an irreversible reaction. 2. Explain how they are...
Give an example of a reversible reaction and an irreversible reaction. 2. Explain how they are fundamentally different. Equilibrium is a dynamic process. Explain what this means. 3. Determine whether the following statements are true or false. Correct the false statements. a. When a chemical reaction reaches equilibrium, the reaction completely stops. b. When a chemical reaction reaches equilibrium, the forward reaction stops and the reverse reaction begins. 4. Determine whether the following statements are true or false. Correct the...
For the reaction 2 NO (g) + O2 (g) → 2 NO2 (g) it is found...
For the reaction 2 NO (g) + O2 (g) → 2 NO2 (g) it is found that the rate doubles when the O2 concentration is doubled, but the rate increases by a factor of 4 when the NO concentration is doubled. Which of the following mechanisms is/are consistent with this? 1. (i) NO + O2 ⇋ NO3 (fast) (ii) NO + NO3 → 2 NO2 (slow) 2. (i) 2 NO → N2O2 (slow) (ii) O2 + N2O2 → N2O4 (fast)...
The reversible gas-phase decomposition of nitrogen tetra oxide, N2O4, to nitrogen dioxide, NO2, is to be...
The reversible gas-phase decomposition of nitrogen tetra oxide,
N2O4, to nitrogen dioxide, NO2, is
to be carried out at constant temperature. The feed consists of
pure N2O4 at 340 K and 202.6 kPa (2 atm). The rate
constant of forward reaction is 0.5 min-1 and the
equilibrium constant, Kc, at 340 K = 0.1
mol/dm3.
N2O4
2NO2
Use POLYMATH, calculate the equilibrium conversion of
N2O4 in a flow reactor.
We were unable to transcribe this imageWe were unable to transcribe...
1) Which statement below regarding the concentration of products for a chemical reaction at equilibrium is...
1) Which statement below regarding the concentration of products for a chemical reaction at equilibrium is true? a) They will not change because the forward and reverse rates are equal b) They will not change because there are no more reactants c) They will not change because this is a constant for each reaction d) They will change continually because of reversibility 2) The law of mass action is a result of: a) limiting reagent stoichiometry b) the law of...
Consider the reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf...
Consider the reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K. ______ kJ (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.45 atm and 1.55 atm, respectively. _____ kJ
What are the units of the rate constant for the following reaction? N2O4(g) ---> 2 NO2(g)...
What are the units of the rate constant for the following reaction? N2O4(g) ---> 2 NO2(g) rate = k(N2O4) Can someone please break this down step by step?
NO2(g) ⇌ N2O4(g) Kp = 11.3 at 25oC (a) Calculate G if the P(NO2) = 0.29 atm, and...
NO2(g) ⇌ N2O4(g) Kp = 11.3 at 25oC (a) Calculate G if the P(NO2) = 0.29 atm, and P(N2O4) = 1.6 atm. (b) Predict the direction in which the reaction will shift to reach equilibrium. Explain how you determined this. (c) Once equilibrium is reached are there more reactants or products present. Explain how you determined this.
The Kc for the reaction at 298 K is given N2O4(g) ⇋ 2 NO2(g) Kc =...
The Kc for the reaction at 298 K is given N2O4(g) ⇋ 2 NO2(g) Kc = 5.9 × 10–3 What is the Kc for the following reaction? ½ N2O4(g) ⇋ NO2(g) Kc = ?
Given the reaction below: N2O4(g)→2NO2(g)N2O4(g)→2NO2(g) d) You increase [NO2][NO2], but change nothing else about the system....
Given the reaction below: N2O4(g)→2NO2(g)N2O4(g)→2NO2(g) d) You increase [NO2][NO2], but change nothing else about the system. How will this affect the value of K? Select one: a. K will decrease. b. K will increase. c. K will not change.
The reversible gas-phase decomposition of nitrogen tetra oxide,
N2O4, to nitrogen dioxide, NO2, is
to be carried out at constant temperature. The feed consists of
pure N2O4 at 340 K and 202.6 kPa (2 atm). The rate
constant of forward reaction is 0.5 min-1 and the
equilibrium constant, Kc, at 340 K = 0.1
mol/dm3.
N2O4
2NO2
Use POLYMATH, calculate the equilibrium conversion of
N2O4 in a flow reactor.
We were unable to transcribe this imageWe were unable to transcribe...
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