The pressure on top of Mt. Everest averages about 235 mmHg. Convert this pressure to

b. psi

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The pressure in Denver. Colorado (elevation 5280 ft). averages about 24.9 in Hg. Convert this pressure to

d. Pa

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The pressure in Denver. Colorado (elevation 5280 ft). averages about 24.9 in Hg. Convert this pressure to

c. psi

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The pressure in Denver. Colorado (elevation 5280 ft). averages about 24.9 in Hg. Convert this pressure to

b. mmHg

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The world record for lowest pressure (at sea level) was 652.5 mmHg recorded inside Typhoon Tip on October 12,1979, in the Western Pacifie Ocean. Convert this pressure to

a. torr

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The pressure on top of Mt. Everest averages about 235 mmHg. Convert this pressure to

a. torr

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The pressure in Denver. Colorado (elevation 5280 ft). averages about 24.9 in mmHg. Convert this pressure to

a. atm

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Which statement is true of a reaction in which ∆*V* is positive? Explain.

a. ∆*H* = ∆*E*

b. ∆*H* > ∆*E*

c. ∆*H* < ∆*E*

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When 1 mol of a gas burns at constant pressure, it produces 2418 J of heat and does 51 of work. Identify ∆*E*, ∆*H*, *q, *and *w *for the process.

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Which expression describes the heat evolved in a chemical reaction when the reaction is carried out at constant pressure? Explain.

a. ∆*E* – *w*

b. ∆*E*

c. ∆*E* – *q*

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The heat of vaporization of water at 373 K is 40.7 kJ/mol. Find *q*, *w*, Δ*E*, and Δ*H* for the evaporation of 454 g of water at this temperature.

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A typical frostless refrigerator uses 655 kWh of energy per year in the form of electricity. Suppose that all of this electricity is generated at a power plant that burns coal containing 3.2% sulfur by mass and that all of the sulfur is emitted as SO_{2 }when the coal is burned. If all of the SO_{2} goes on to react with rainwater to form H_{2}SO_{4}, what mass of H_{2}SO_{4} does the annual operation of the refrigerator produce? (Hint: Assume that the remaining percentage of the coal is carbon and begin by calculating Δ*H*°_{rxn} for the combustion of carbon.)

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When 10.00 g of phosphorus is burned in O_{2}(*g*) to form P_{4}O_{10}(*s*), enough heat is generated to raise the temperature of 2950 g of water from 18.0 °C to 38.0 °C. Calculate the enthalpy of formation of P_{4}O_{10}(*s*) under these conditions.

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What is a manometer? How does it measure the pressure of a sample of gas?

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What are the Arrhenius definitions of an acid and a base?

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Explain how a strong electrolyte, a weak electrolyte, and a nonelectrolyte differ.

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Without doing any calculations, determine which element in each of the compounds will have the highest mass percent composition.

d. NH_{3}

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Without doing any calculations, determine which element in each of the compounds will have the highest mass percent composition.

c. C_{6}H_{12}O_{6}

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Without doing any calculations, determine which element in each of the compounds will have the highest mass percent composition.

b. N_{2}O

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a. CO

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The elements X and Y form a compound that is 40% X and 60% Y by mass. The atomic mass of X is twice that of Y. What is the empirical formula of the compound?

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A mixture of 50.0 g of S and 1.00 X 10 ^{2} g of Cl_{2} reacts completely to form S_{2}CI_{2} and SCI_{2}. Find the mass of S_{2}CI_{2} formed.

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A sugar crystal contains approximately 1.8 x 10^{17 }sucrose (C_{12}H_{22}O_{11}) molecules. What is its mass in mg?

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Calculate the mass (in g) of each sample.

c. 1 water molecule

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Calculate the mass (in g) of each sample.

b. 9.85 x 10^{19 }CCl_{2}F_{2 }molecules

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