Conversion of Units
#4) A typical barometric pressure in Redding, CA, is 750 mmHg. Calculate the pressure in atm and kPa.
0.987 atm
99.99 kPa
#28) What is the temperature of an 11.2 L sample of carbon monoxide, CO, at 744 torr if it occupies 13.3 L at 55oC and 744 torr.
276.2 K or 3.2oC
#65) Joseph Priestley first prepared pure oxygen by heating mercuric oxide, HgO:
2HgO(s) ⟶ 2Hg(l)+O2(g)
What volume of O2 at 23 °C and 0.975 atm is produced by the decomposition of 5.36 g of HgO?
0.309 L
#6) A typical barometric reading in Kansas City is 740 torr. What is the reading in atm, mmHg, and kPa?
0.974 atm
740 mmHg
98.67 kPa#29) A 2.50 L volume of hydrogen measured at -196oC is warmed to 100oC. Calculate the volume of gas at the higher temperature, assuming no change in pressure.
12.11 L
#66) 4H2O + 3Fe ---> Fe3O4 + 4H2
What volume of H2 at a pressure of 745 torr and a temperature of 200C can be prepared from the reaction of 15 g of H2O?
20.37 L
#7) Canadian tire pressure gauges are read in kilopascals. What reading in kPa corresponds to 32 psi?
**1 psi= 6.89476 kPa**
220.632 kPa
#32) The volume of an automobile air bag was 66.8 L when inflated at 25oC with 77.8 g of nitrogen gas. What was the pressure in the bag in kPa?
103.15 kPa
#67) CCl2F2 + 4H2 ---> CH2F2 + 2HCl
What volume of hydrogen at 225 atm and 35.50C would be required to react with 1 ton (1.000x103 kg) of CCl2F2 ?
3724.34 L
#33) How many mols of BF3 are contained in 4.3410 L bulb at 788 K if the pressure is 1.220 atm? How many grams of BF3?
0.0819 mol
5.55 g
#78) Each molecule of hemoglobin combines with four molecules of O2. If 1.00g hemoglobin combines with 1.53 mL O2 at 37oC and 743 torr, what is the molar mass of hemoglobin?
68,027 g/mol