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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 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. ∆Ew

b. ∆E

c. ∆Eq

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The heat of vaporization of water at 373 K is 40.7 kJ/mol. Find q, w, ΔE, and ΔH 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 SOwhen the coal is burned. If all of the SO2 goes on to react with rainwater to form H2SO4, what mass of H2SO4 does the annual operation of the refrigerator produce? (Hint: Assume that the remaining percentage of the coal is carbon and begin by calculating ΔH°rxn for the combustion of carbon.) 

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When 10.00 g of phosphorus is burned in O2(g) to form P4O10(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 P4O10(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. NH3

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

c. C6H12O6

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

b. N2O

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

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 Cl2 reacts completely to form S2CI2 and SCI2. Find the mass of S2CI2 formed. 

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A sugar crystal contains approximately 1.8 x 1017 sucrose (C12H22O11) 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 1019 CCl2Fmolecules

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