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( Q1 ) Convert 562 mmHg to atm. 1 atm = 760 mmHg. 0.739 atm.
( Q2 ) Convert 606 mmHg to atm and kPa? 1 atm = 760 mmHg = 1.01325 x 10^5 Pa (SI unit) = 101.325 kPa. 0.797 atm; 80.8 kPa.
( Q3 ) A gas occupying a volume of 725 mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0. atm. What is its final volume? 1300 mL.
( Q4 ) At 46°C a sample of ammonia gas exerts a pressure of 5.3 atm. What is the pressure when the volume of the gas is reduced to one-tenth (0.10) of the original value at the same temperature? Suppose V 1 = 10 mL then V 2 = 1 mL. 53 atm.
( Q5 ) A sample of air occupies 3.8 L when the pressure is 1.2 atm. (The temperature is kept constant). (a) What volume does it occupy at 6.6 atm? 0.691 L. (b) What pressure is required in order to compress it to 0.075 L? 60.8 atm.
( Q6 ) Under constant-pressure conditions a sample of hydrogen gas initially at 88°C and 9.6 L is cooled until its final volume is 3.4 L. What is its final temperature? 127.85 K (-145.15oC).
( Q7 ) Given that 6.9 moles of carbon monoxide gas are present in a container of volume 30.4 L, what is the pressure of the gas (in atm) if the temperature is 62°C? 6.23 atm.
( Q8 ) A certain amount of gas at 25°C and at a pressure of 0.800 atm is contained in a glass vessel. Suppose that the vessel can withstand a pressure of 2.00 atm. How high can you raise the temperature of the gas without bursting the vessel? 745 K.
( Q9 ) The temperature of 2.5 L of a gas initially at STP is raised to 250°C at constant volume. Calculate the final pressure of the gas in atm. STP (P = 1 atm; T = 273 K) 1.92 atm.
( Q10 ) A gas evolved during the fermentation of glucose has a volume of 0.78 L at 20.1°C and 1.00 atm. What was the volume of this gas at the fermentation temperature of 36.5°C and 1.00 atm pressure? 0.824 L.
( Q11 ) Calculate the volume (in liters) of 88.4 g of CO 2 at STP. n = 88.4 / 44 = 2.01 mol 45 L.
( Q12 ) Dry ice is solid carbon dioxide. A 0.050-g sample of dry ice is placed in an evacuated 4.6-L vessel at 30°C. Calculate the pressure inside the vessel after all the dry ice has been converted to CO 2 gas. 6.14 x 10-3^ atm.
( Q13 ) At 741 torr and 44°C, 7.10 g of a gas occupy a volume of 5.40 L. What is the molar mass of the gas? 35 g/mol.
( Q19 ) A mixture of helium and neon gases is collected over water at 28.0°C and 745 mmHg. If the partial pressure of helium is 368 mmHg, what is the partial pressure of neon? (Vapor pressure of water at 28°C 5 28.3 mmHg). 349 mmHg (0.459 atm).
( Q20 ) A sample of ammonia (NH 3 ) gas is completely decomposed to nitrogen and hydrogen gases over heated iron wool. If the total pressure is 866 mmHg, calculate the partial pressures of N 2 and H 2. H 2 : 650 mmHg. N 2 : 217 mmHg.
( Q21 ) A sample of zinc metal reacts completely with an excess of hydrochloric acid: Zn(s) + 2HCl(aq) → ZnCl 2 (aq) + H 2 (g) The hydrogen gas produced is collected over water at 25.0°C. The volume of the gas is 7.80 L, and the pressure is 0.980 atm. Calculate the amount of zinc metal in grams consumed in the reaction. (Vapor pressure of water at 25°C 5 23.8 mmHg). 19.8 g.
