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Question
According to the first law of thermodynamics, the energy of the universe is constant. Does this mean that
E is always equal to zero?A) No,
E does not always equal zero, but this is due only to factors such as friction and heat.B) No,
E never equals zero because energy is always flowing between the system and the surroundings.C) No,
E does not always equal zero because it refers to the system's internal energy, which is affected by heat and work.D) Yes,
E= 0 at all times, which is why q= -w.E) No,
E never equals zero because work is always being done on the system or by the system. Answer
This answer is hidden. It contains 1 characters.
Related questions
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B) The abundance of 7Li is less than 6Li.
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D) Not enough data is provided to determine the correct answer.
E) Based on the atomic mass, only 7Li occurs naturally.
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Which of the following atomic symbols represents an isotope of ?
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Q:
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B) Atoms 1 and 2 must be isotopes.
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Q:
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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.
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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:
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Q:
A reaction that is second-order in one reactant has a rate constant of 2.2 x 10-2L/(mols). If the initial concentration of the reactant is 0.360 mol/L, how long will it take for the concentration to become 0.180 mol/L?A) 320 sB) 63 sC) 1300 sD) 32 sE) 130 s
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