Riverside City College Chemistry Conversions Questions

Description

1.

Perform the conversions.

691.1 mmHg=

atm

1.135 atm=

Torr

650.5 kPa=

atm

867.3 mmHg=

Pa

2.

The pressure of a sample of argon gas was increased from 1.86 atm to 6.70 atm at constant temperature. If the final volume of the argon sample was 11.1 L, what was the initial volume of the argon sample? Assume ideal behavior.

?=

L

3.

A sample of oxygen gas initially at 383 K

was heated to 437 K. If the volume of the oxygen gas sample at 437 K is 738.8 mL,what was its volume at 383 K?

?=

mL

4.

A sample of xenon gas occupies a volume of 7.61 L

at 441 K. If the pressure remains constant, at what temperature will this same xenon gas sample have a volume of 4.43 L?

?=

K

5.

An ideal gas in a sealed container has an initial volume of 2.60 L. At constant pressure, it is cooled to 17.00 ?C, where its final volume is 1.75 L. What was the initial temperature?

?1=

?C

6.

A sample of an ideal gas has a volume of 2.30 L

at 288 K and 1.11 atm. Calculate the pressure when the volume is 1.88 L and the temperature is 301 K.

?=

atm

7.

A gas?filled weather balloon has a volume of 58.0 L at ground level, where the pressure is 755 mmHg and the temperature is 22.0 ?C. After being released, the balloon rises to an altitude where the temperature is ?5.71 ?C and the pressure is 0.0702 atm.What is the weather balloon’s volume at the higher altitude?

?=

L

8.

A 3.53 mol sample of freon gas was placed in a balloon. Adding 3.50 mol of freon gas to the balloon increased its volume to 15.8 L. What was the initial volume of the balloon?

?=

L

9.

If 86.5 mol of an ideal gas is at 3.73 atm and 309 K, what is the volume of the gas?

volume:

L

10.

If an ideal gas has a pressure of 7.49 atm, a temperature of 443 K, and a volume of 97.37 L, how many moles of gas are in the sample?

?=

mol

11.

What pressure is exerted by 949.9 g of CH4 in a 0.550 L steel container at 174.7 K?

?=

atm

12.

How many moles of N2 are in a 2.90 L cylinder at 77.3 °C and 9.45 atm ?

moles of N2:

13.

What volume is occupied by 0.309 mol of CO2 at 281.6 K and 719 mmHg?

?=

L

14.

What pressure is exerted by 0.140 mol N2 in a 5.87 L steel container at 84.5 °C?

?=

atm

15.

How many grams of Kr

are in a 3.51 L cylinder at 44.8 ?C and 4.55 atm?

mass:

g

16.

If 2.94 g Ar are added to 2.43 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of the resulting gaseous mixture?

?total=

atm

17.

A mixture of He,

Ne, and Ar has a pressure of 11.0 atm at 28.0 °C. If the partial pressure of He is 3.59 atm and the partial pressure of Ar is 2.47 atm, what is the partial pressure of Ne?

?Ne=

atm

18.

A sample of nitrogen gas was collected via water displacement. Since the nitrogen was collected via water displacement, the sample is saturated with water vapor. If the total pressure of the mixture at 21 °C is 1.34 atm, what is the partial pressure of nitrogen? The vapor pressure of water at 21 °C is 18.7 mm Hg.

atm

19.

In the reaction, 

2HgO(s)?2Hg(s)+O2(g)

what mass of mercury(II) oxide, HgO, would be required to produce 981 L of oxygen, O2, measured at STP?

mass:

g

20.

In the reaction, 

2HgO(s)?2Hg(s)+O2(g)

how many liters of oxygen, O2, measured at STP, would be produced from the decomposition of 145 g of mercury(II) oxide, HgO?

O2 produced:

L

21.

When aluminum reacts with concentrated hydrochloric acid, hydrogen gas is produced.

2Al(s)+6HCl(aq)?2AlCl3(aq)+3H2(g)

What mass of Al(s) is required to produce 723.0 mL  of H2(g) at STP?

mass:

g Al