9.30Perform the following pressure conversions.
(a)1.15 atm to torr
(b)968 torr to atm
(c)2.50 × 105 Pa to atm
(d)695 mm Hg to torr
(e)0.953 atm to Pa
(f)653 torr to mm Hg
(g)1545 mm Hg to Pa
(h)3.73 kPa to atm
9.38Given a fixed quantity of a gas at constant temperature, calculate the new volume the gas would occupy if the pressure were changed as shown in the following table.
Hint:
9.41What pressure is required to compress 925 L of N2 at1.25 atm into a container whose volume is 6.35 L?
9.42What will be the final volume of 186 mL of Cl2 if the pressure increases from 0.945 atm to 1.76 atm?
9.49For a fixed amount of gas held at constant pressure, calculate the new volume the gas would occupy if the temperature were changed as shown in the following table.
Hint: T must be in Kelvin!
9.50For a fixed amount of gas held at constant pressure, calculate the new volume the gas would occupy if the temperature were changed as shown in the following table.
Hint:
T must be in Kelvin!
9.51For a fixed amount of gas held at constant pressure, calculate the temperature in degrees Celsius to which the gas would have to be changed to achieve the change in volume shown in the following table.
Hint:
9.64For a gas under a given initial set of conditions, calculate the final value for the variable indicated if the other two variables change as described in the following table.
Hint:
9.71Given the following volumes of gases at STP, calculate the number of moles of each gas and the mass of the gas.
(a) 8.62 L CH4
(b) 350.0 mL Xe
(c) 48.1 L CO
9.75Given the following amounts of gases, calculate the number of moles of each gas. Calculate the volume each amount of gas would occupy at STP.
(a) 5.8 g NH3
(b) 48 g O2
(c) 10.8 g He
9.90Calculate the density in grams per liter of the following gases at STP.
Hint:
(a) NO
(b) NO2
(c) O2
9.91Calculate the density in grams per liter of the following gases at 25.0°C and 735 torr.
Hint:
(a) NH3
(b) N2
(c) N2O
9.98A total of 0.400 L of hydrogen gas is collected over water at 18°C. The total pressure is 742 torr. If the vapor pressure of water at 18°C is 15.5 torr, what is the partialpressure of hydrogen?
9.99A tank contains 78.0 g of N2 and 42.0 g of Ne at a total pressure of 3.75 atm and a temperature of 50.0°C.
Calculate the following quantities.
(a) moles of N2
(b) moles of Ne
(c) partial pressure of N2
(d) partial pressure of Ne
9.118When nitric acid is synthesized from ammonia, the firststep in the process is
4NH3(g) + 5O2(g)4NO(g) + 6H2O(g)
What volume of NO at STP can be formed from 1250 L of NH3 at 325°C and 4.25 atm, assuming temperature andpressure conditions remain constant?
9.120Nitric oxide is produced in the reaction between copper metal and nitric acid:
3Cu(s) + 8HNO3(aq) 3Cu(NO3)2(aq) + 4H2O(l) + 2NO(g)
What mass of copper is required to produce 15.0 L of NO at 725 torr and 20.0°C?