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Concept explainers
(a)
Interpretation:
The electronic configuration for the given orbital diagram has to be given.
The given orbital diagram is,
Figure 1
Concept Introduction:
Aufbau’s principle:
Aufbau’s principle states that electrons are filled into atomic orbitals in the increasing order of orbital energy level. According to the Aufbau principle the available atomic orbitals with the lowest energy levels are occupied before those with higher energy levels.
Figure 2
(b)
Interpretation:
The electronic configuration for the given orbital diagram has to be given.
The given orbital diagram is,
Figure 3
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The electronic configuration for the given orbital diagram has to be given.
The given orbital diagram is,
Figure 4
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
The electronic configuration for the given orbital diagram has to be given.
The given orbital diagram is,
Figure 5
Concept Introduction:
Refer to part (a).
(e)
Interpretation:
The electronic configuration for the given orbital diagram has to be given.
The given orbital diagram is,
Figure 6
Concept Introduction:
Refer to part (a).
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Chapter 10 Solutions
FOUND.OF COLLEGE CHEMISTRY
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- A metal cylinder with a capacity of 6.0 L is filled with compressed propane (C3H8). The pressure and temperature of the cylinder when it was initially filled were 120 atm and 75 ◦C, respectively. The molar mass of carbon is 12 g·mol−1 and the molar mass of hydrogen is 1 g·mol−1. a) How many moles of propane are in the cylinder? b) What is the mass of the propane inside the cylinder? c) After some time, the cylinder and its contents cool to 25 ◦C. What is the pressure in the cylinder after it has cooled?arrow_forwardThe partial pressure of water vapor in saturated air at 34 °C is 5.25×10-2 atm. (a) How many molecules of water are in 1.16 cm3 of saturated air at 34 °C? (b) What volume of saturated air at 34 °C contains 0.563 mol of water?arrow_forwardA gas mixture being used to simulate the atmosphere of another planet consists of 320 mg of methane, 175 mg of argon, and 225 mg of nitrogen. The partial pressure of nitrogen at 300 K is 15.2 kPa. Calculate (a) the volume and (b) the total pressure of the mixture.arrow_forward
- Sulfur dioxide reacts with oxygen in the presence of plati- num to give sulfur trioxide: 2 SO2(g) + O2(g) → 2 SO3(g) Suppose that at one stage in the reaction, 26.0 mol SO2, 83.0 mol O2, and 17.0 mol SO3 are present in the reaction vessel at a total pressure of 0.950 atm. Calculate the mole fraction of SO3 and its partial pressure.arrow_forwardThe partial pressure of oxygen in a mixture of oxygen andhydrogen is 0.200 atm, and that of hydrogen is 0.800 atm.(a) How many molecules of oxygen are in a 1.500-L container of this mixture at 40°C?(b) If a spark is introduced into the container, how many grams of water will be produced?arrow_forwardA 6.53-g sample of a mixture of magnesium carbonateand calcium carbonate is treated with excesshydrochloric acid. The resulting reaction produces 1.72 Lof carbon dioxide gas at 28 °C and 743 torr pressure.(a) Write balanced chemical equations for the reactionsthat occur between hydrochloric acid and each componentof the mixture. (b) Calculate the total number ofmoles of carbon dioxide that forms from these reactions.(c) Assuming that the reactions are complete, calculatethe percentage by mass of magnesium carbonate in themixture.arrow_forward
- A 0.564 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H,SO,(aq) MSO,(aq) + H, (g) → A volume of 219 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal. molar mass: g/mol * TOOLS x10"arrow_forwardA student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.arrow_forwardThe van der Waals constants for HCl are a = 3.67 atm·liter2·mole–2, and b = 40.8 cc·mole–1. Find the critical constants of this substance.arrow_forward
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- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
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