1.A bicycle tire is filled to a pressure of 4.42 atm (65 psi) at a temperature of 12?C. If the temperature of the tire increases to 33?C, what is the pressure in the tire? Assume the volume of the tire is constant.2.If 8.5 g of oxygen gas (O2) is introduced into an evacuated 1.50 L flask at 22?C, what is the pressure inside the flask?3.A tightly sealed 4.0-L flask contains 884 mm Hg of N2 at 94.0?C. The flask is cooled until the pressure is reduced 442 mm Hg. What is the temperature of the gas?4.
1. A bicycle tire is filled to a pressure of 4.42 atm (65 psi) at a temperature of 12?C. If the temperature of the tire increases to 33?C, what is the pressure in the tire? Assume the volume of the tire is constant.
2. If 8.5 g of oxygen gas (O2) is introduced into an evacuated 1.50 L flask at 22?C, what is the pressure inside the flask?
3. A tightly sealed 4.0-L flask contains 884 mm Hg of N2 at 94.0?C. The flask is cooled until the pressure is reduced 442 mm Hg. What is the temperature of the gas?
4. If aqueous solutions of nickel(II) chloride and potassium phosphate are mixed, which insoluble compound will form?
5. Which of the following ionic compounds is not soluble in water?
6. Which of the following ionic compounds are likely to be soluble in water: Mg(OH)2, Pb(NO3)2, AgI, Na2CO3, and Cu3(PO4)3
7. A barometer is filled with a cylindrical column of mercury that is 76.0 cm high and 1.000 cm in diameter. If the density of mercury is 13.53 g/cm3 what is the mass of mercury in the column?
8. Calcium carbonate, or limestone is relatively insoluble in water. At 25 C only 5.8 mg will dissolve in 1.0 liter of water. What volume of water is needed to dissolve 5.0g of calcium carbonate?
Document Preview: 1. A bicycle tire is filled to a pressure of 4.42 atm (65 psi) at a temperature of 12?C. If the temperature of the tire increases to 33?C, what is the pressure in the tire? Assume the volume of the tire is constant.
2. If 8.5 g of oxygen gas (O2) is introduced into an evacuated 1.50 L flask at 22?C, what is the pressure inside the flask?
3. A tightly sealed 4.0-L flask contains 884 mm Hg of N2 at 94.0?C. The flask is cooled until the pressure is reduced 442 mm Hg. What is the temperature of the gas?
4. If aqueous solutions of nickel(II) chloride and potassium phosphate are mixed, which insoluble compound will form?
5. Which of the following ionic compounds is not soluble in water?
6. Which of the following ionic compounds are likely to be soluble in water: Mg(OH)2, Pb(NO3)2, AgI, Na2CO3, and Cu3(PO4)3
7. A barometer is filled with a cylindrical column of mercury that is 76.0 cm high and 1.000 cm in diameter. If the density of mercury is 13.53 g/cm3 what is the mass of mercury in the column?
8. Calcium carbonate, or limestone is relatively insoluble in water. At 25 C only 5.8 mg will dissolve in 1.0 liter of water. What volume of water is needed to dissolve 5.0g of calcium carbonate?