# chem

75L stainless steel container was charged with 3 atm of hydrogen gas and 4 atm of oxygen gas. a spark ignited the misture, producing water. what is the pressure of the tank at 25C? at 125C?

1. 👍
2. 👎
3. 👁
4. ℹ️
5. 🚩
1. The 3 atm (partial pressure) of H2 will combine with 1.5 atm (partial pressure) of O2 to produce 3 atm (partial pressure) of H2O, with 2.5 atm (partial pressure) of O2 left over. Thus 7 atm of reactants produces 5.5 atm of products + unreacted O2.

I am assuming that the inital and final temperatures are what you have specified. This means that the heat of reaction will have been transfered out, as would be the case with a calorimeter. In that situation, with constant T and volume, the final pressure is proportional to the number of moles present, and that factor is 5.5/7 = 0.7857, at both temperatures.

1. 👍
2. 👎
3. ℹ️
4. 🚩
2. I made a mistake in my previous answer by not considering the condensation of H2O. At 25C, almost all of the H20 produced will be in liquid form, so the actual pressure of the gas after cooling down the reaction products to 25 C will be 2.5/7 = 35.7% of the initial pressure. At 125 C, most (but not all) of the H2O produced by combustion will be in gaseous form. You will have to make use of data on the saturation pressure of H2O to get exact answers.

1. 👍
2. 👎
3. ℹ️
4. 🚩

## Similar Questions

1. ### chem.

A sample of argon at 300. °C and 50.0 atm pressure is cooled in the same container to a temperature of 0. °C. What is the new pressure? 105 atm 45.5 atm 54.9 atm 23.8 atm 42.7 atm

2. ### Chemistry

Consider the following reaction. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a pressure of 0.724 atm , and N2O4 at a pressure of 0.0524 atm . The volume of the container is then reduced to half its

3. ### Chemistry

Consider an ideal gas encloesd in a 1.00 L container at an internal pressure of 10.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 20.0 L. w = ____ J now

4. ### Chemistry

A 0.65 mole quantity of O2 occupies 4.0 L at 20.◦C. What is the final pressure exerted by the gas? 1. 0.92 atm 2. 3.9 atm 3. 6.2 atm 4. 1.1 atm 5. 0.27 atm — Initially, I got .27 atm. I got this answer by plugging in the

1. ### Chemistry

A rigid cylinder contains a sample of gas at STP. What is the pressure of this gas after the sample is heated to 410 K? a. 1.0 atm b. 0.50 atm c. 0.67 atm d. 1.5 atm Explain how you get the answer.

2. ### chemistry

Four gases were combined in a gas cylinder with these partial pressures: 3.5 atm N2, 2.8 atm O2, 0.25 atm Ar, and 0.15 atm He.What is the mole fraction of N2 in the mixture?

3. ### Chemistry (Check)

If a gas in a closed container is pressurized from 12 atm to 25 atm and tis original temperature was 32 degrees C, what would the final temperature of the gas be? Tf = 635 K

4. ### chemistry

The pressure inside a hydrogen-filled container was 2.10 atm at 21 C . What would the pressure be if the container was heated to 86 C? Pfinal = ?? atm

1. ### cleveland state university

A sample of gas at 1.3 atm of pressure is in a 2.0 L container. What will the pressure be if the sample is transferred to a 0.90 L container? 1. 0.59 atm 2. 1.4 atm 3. 2.9 atm 4. 3.2 atm

2. ### Chemistry

The partial pressures of the gases in the container are monitored at constant temperature and recorded in the table below. At time t4, is the rate of the reverse reaction greater than, less than, or equal to the rate of the

3. ### chemistry

17 liters of a gas is at an initial temperature of 67 degrees C and a pressure of 88.89 atm, what will be the pressure of the gas if the tempetature of the gas is raised to 94 degrees C and the volume of the gas is decreased to 12

4. ### Chemistry

The number of moles of hydrogen gas present in a 1500 mL container at 298 K and 2.0 atm pressure is?