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Question
Which of the following statements concerning a sample of oxygen gas at 1.00 atm pressure is incorrect?A) The molecules are in constant rapid random motion.
B) The pressure exerted by gaseous oxygen is due to the impact of the molecules with the walls of the container.
C) The average kinetic energy of the gaseous oxygen is inversely proportional to the absolute temperature of the gas.
D) The volume occupied by the oxygen molecules is negligible compared with the size of the container.
E) Collisions between the gaseous molecules are elastic.
Answer
This answer is hidden. It contains 1 characters.
Related questions
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All of the following elements are best classified as metalloids except
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B) Te.
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D) B.
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Q:
Lithium has two naturally occurring isotopes, 6Li and 7Li . The average atomic mass of lithium is 6.941. Which of the following statements concerning the relative abundance of each isotope is correct?
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B) The abundance of 7Li is less than 6Li.
C) The abundance of 6Li is equal to the abundance of 7Li.
D) Not enough data is provided to determine the correct answer.
E) Based on the atomic mass, only 7Li occurs naturally.
Q:
Which of the following atomic symbols represents an isotope of ?
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Q:
Suppose atom 1 has the same number of protons as atom 2, and atom 2 has the same number of neutrons as atom 3. Atom 1 does not have the same number of neutrons as atom 3. Which of the following statements is true?
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B) Atoms 1 and 2 must be isotopes.
C) Atoms 1 and 3 must be isotopes.
D) Atom 2 must have the same number of neutrons as atom 1.
E) Atom 3 must have the same number of protons as atom 1.
Q:
The number of protons in a given nucleus determines the
A) mass number.
B) atomic number.
C) number of electrons.
D) number of protons.
E) number of isotopes.
Q:
If the Thomson model of the atom had been correct, Rutherford would have observed
A) alpha particles bouncing off the foil.
B) alpha particles going through the foil with little or no deflection.
C) alpha particles greatly deflected by the metal foil.
D) positive particles formed in the foil.
E) None of the above observations is consistent with the Thomson model of the atom.
Q:
A subatomic particle is
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Q:
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A) N2(g) + 3H2(g) 2NH3(g)
B) CO(g) + H2O(g) CO2(g) + H2(g)
C) CO(g) + 3H2(g) CH4(g) + H2O(g)
D) CaO(s) + CO2(g) CaCO3(s)
E) HBr(g) H2(g) + Br2(l)
Q:
For the reaction 2NO(g) + O2(g) 2NO2(g) at 750ºC, what is the relationship between Kc and Kp?A) Kc= KpB) Kc= Kp x (RT)-1C) Kc= Kp= 1.0D) Kc= Kp x (RT)E) Kc= Kp x (RT)1
Q:
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Q:
Which of the following represents a dynamic equilibrium?
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Q:
For the hypothetical reaction A → products, the concentration of A was monitored over time. From the following graph, what is the rate constant for the decomposition of A?A) -0.02735 s-1B) 2.3026 s-1C) -2.3026 s-1D) 0.02735 s-1E) 0.01188 s-1
Q:
Which of the following corresponds to the correct equation for the half-life of a first-order reaction?A) B) C) D) E)
Q:
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Q:
A second-order reaction starts with an initial concentration of 0.100 mol/L of the reactant. If the rate constant is 3.6 x 10-2L/(mol·s), what is the time required to decrease the initial concentration to 0.050 mol/L?A) 280 sB) 420 sC) 19.3 sD) 1.39 sE) 830 s
Q:
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Q:
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Q:
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Q:
The reaction between selenous acid and the iodide ion in acid solution isH2SeO3(aq) + 6I-(aq) + 4H+(aq) → Se(s) + 2I3-(aq) + 3H2O(l)The data in the following table were measured at 0C. Experiment[H2SeO3]0(M)[H+]0(M)[I-]0(M)Initial Rate [mol/(L·s)]11.00 x 10-42.00 x 10-23.00 x 10-25.30 x 10-722.00 x 10-42.00 x 10-23.00 x 10-21.06 x 10-633.00 x 10-44.00 x 10-23.00 x 10-26.36 x 10-643.00 x 10-48.00 x 10-23.00 x 10-22.54 x 10-553.00 x 10-48.00 x 10-26.00 x 10-22.04 x 10-462.00 x 10-42.00 x 10-26.00 x 10-28.48 x 10-6Tripling the initial concentration of H2SeO3while holding the initial concentrations of H+ and I- constant increases the rate of the reaction by a factor ofA) 8.B) 4.C) 3.D) 2.E) 1.
Q:
The reaction between selenous acid and the iodide ion in acid solution isH2SeO3(aq) + 6I-(aq) + 4H+(aq) → Se(s) + 2I3-(aq) + 3H2O(l)The data in the following table were measured at 0C. Experiment[H2SeO3]0(M)[H+]0(M)[I"]0(M)Initial Rate [mol/(L·s)]11.00 x 10-42.00 x 10-23.00 x 10-25.30 x 10-722.00 x 10-42.00 x 10-23.00 x 10-21.06 x 10-633.00 x 10-44.00 x 10-23.00 x 10-26.36 x 10-643.00 x 10-48.00 x 10-23.00 x 10-22.54 x 10-553.00 x 10-48.00 x 10-26.00 x 10-22.04 x 10-462.00 x 10-42.00 x 10-26.00 x 10-28.48 x 10-6What is the rate constant for this reaction?A) 1.5 x 104L5/(mol5·s)B) 1.5 x 1010L5/(mol5·s)C) 4.9 x 105L5/(mol5·s)D) 294 L5/(mol5·s)E) 8.8 L5/(mol5·s)
Q:
For the reaction A + B + C → products, the following initial-rate data were obtained. [A]0(mol/L)[B]0(mol/L)[C]0(mol/L)Initial Rate (mol/(L·s))0.400.400.200.01600.200.400.400.00800.600.100.200.00150.200.100.200.00050.200.200.400.0020What are the reaction orders with respect to A, B, and C, respectively?A) 0, 1, 1B) 1, 2, 1C) 1, 1, 1D) 1, 2, 0E) 0, 2, 1
Q:
Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine:2NO(g) + Cl2(g) → 2NOCl(g)The following initial rates at a given temperature were obtained for the concentrations listed below. ExperimentInitial Rate (mol·L-1·h-1)[NO]0(mol·L-1)[Cl2]0(mol·L-1)12.210.250.25219.890.750.2536.630.250.75From the data, what is the experimental rate law?A) Rate = k[Cl2]B) Rate = k[NO]C) Rate = k[NO][Cl2]2D) Rate = k[NO]2[Cl2]E) Rate = k[NO][Cl2]1/2
Q:
If a reaction is first-order with respect to a particular reactant, when the concentration of that reactant is increased by a factor of 2, the reaction rate will _____.
A) increase by a factor of 2.
B) remain constant.
C) decrease by a factor of .
D) decrease by a factor of .
E) increase by a factor of 4.
Q:
For a certain first-order reaction with the general form aA → products, the rate is 0.32 M·s-1 when the concentration of the reactant is 0.29M. What is the rate constant for this reaction?A) 0.26 s-1B) 1.1 s-1C) 0.32 s-1D) 3.1 s-1E) 3.8 s-1