Oxygen collection over water

The total pressure of a 200-mL sample of oxygen collected over water at 25 °C is 1.030 atm. (a) How many moles of gas is present (b) How many moles of oxygen is present (c) How many moles of water vapor is present ... [Pg.199]

A 250 ml flask is filled with oxygen, collected over water at a barometric pressure of 730 torr and a temperature of 25°C. What will be the volume of the oxygen sample, dry, at standard conditions ... [Pg.164]

What is the pressure of oxygen collected over water at 17°C if the total pressure of the system is 735 torr and the vapor pressure of water at this temperature is 15 torr ... [Pg.82]

What volume of oxygen, collected over water, will be obtained at 23°C and 762 torr barometric pressure from the thermal decomposition of 0.0600 mol of KCIO3 ... [Pg.345]

Determine the volume of oxygen collected over water at 25°C and 762 torr barometric pressure by decomposition of 1.00 g of KCIO3 (PH2O = 24 torr). [Pg.102]

Problem 5.41. The total pressure in a vessel containing oxygen collected over water at 25 °C was 723 torr. The vapor pressure of water at that temperature is 23.8 torr. What was the pressure of the gas ... [Pg.116]

A 1.500-g sample containing sodium nitrate was heated to form NaN02 and 02. The oxygen evolved was collected over water at 23°C and 752 mm Hg its volume was 125.0 mL. Calculate the percentage of NaN03 in the sample. The vapor pressure of water at 23°C is 21.07 mm Hg. [Pg.576]

Self-Test 4.13A As a sample of oxygen was collected over water at 24°C and 745 Torr, it became saturated with water vapor. At this temperature, the vapor pressure of water is 24.38 Torr. What is the partial pressure of the oxygen ... [Pg.278]

Another type of gas law problem involves stoichiometry. Gas stoichiometry problems are just like all other stoichiometry problems—you must use moles. In addition, one or more gas laws are necessary. Let s look at a gas stoichiometry problem. What volume, in liters of oxygen gas, collected over water, forms when 12.2 g ofKCl03 decompose according to the following equation ... [Pg.92]

First, you need to determine the pressure of just the oxygen gas. It was collected over water, so the total pressure of 755.0 torr is the sum of the partial pressures of the oxygen and the water vapor ... [Pg.111]

The liberated oxygen is collected over water. The reaction occurs at room temperature. [Pg.43]

Exactly 100 cm3 of oxygen are collected over water at 23°C and 800 torr. Compute the standard volume (volume at S.T.P.) of the dry oxygen. Vapor pressure of water at 23°C is 21.1 torr. [Pg.71]

Oxygen is generated by heating potassium chlorate, and its weight is determined by the loss in weight of that material. Since the gas is collected over water, under the conditions of temperature and pressure prevailing in the laboratory, the volume must be corrected to standard conditions by means of the formula on page 44. [Pg.25]

Sample Oxygen gas is collected over water at 28°C. The total pressure of the sample is 785 mm Hg. At 28°C, the vapor pressure of water is 28 mm Hg. What pressure is the oxygen gas exerting ... [Pg.160]

A student collected 375 mL of oxygen gas from the decomposition of hydrogen peroxide. The gas was collected over water at 19X1 and 100.2 kPa. What mass of oxygen was collected The vapour pressure of water at 19 is 2.2 kPa. [Pg.651]

Oxygen gas is collected over water in an apparatus such as that shown in Figure 12.8 at a barometric pressure of 759 torr at 23°C. [Pg.345]

Calculate the volume of oxygen gas, collected over water at 836 torr barometric pressure and 298 K, that can be prepared by the thermal decomposition of 2.40 g of KC103.(Pwater = 24 torr at25°C)... [Pg.328]

At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22° and a pressure of 734 torr. Calculate the mass percent ... [Pg.182]

A sample of mercuric oxide. weighing 2.000 g is strongly heated in a test tube and the volume of oxygen evolved is measured. What would be the predicted volume of the e olved gas if the atmospheric pressure was 745 mm of mercury, the temperature was 28.5 C, and the gas was collected over water ... [Pg.572]

A certain mass of oxygen was collected over water when potassium chlorate was decomposed by heating. The volume of the oxygen sample collected was 720 mL at 25°C and a barometric pressure of 755 torn What would the volume of the oxygen be at STP (Hint First calculate the partial pressure of the oxygen. Then use the combined gas law.)... [Pg.884]

Ten pounds of KCIO3 is completely decomposed and the oxygen evolved collected over water at 80 F. The barometer reads 29.7 in. Hg. What weight of saturated oxygen is obtained ... [Pg.310]

Example 3 220 mL of oxygen was collected over water. The total pressure of oxygen plus water vapor was 745.8 mmHg at 25°C (298 K). How many moles of oxygen gas were collected ... [Pg.314]

The oxygen gas can be collected over water, as shown in Figure 5.13. Initially, the inverted bottle is completely filled with water. As oxygen gas is generated, the gas bubbles rise to the top and displace water from the bottle. This method of collecting a gas is based on the assumptions that the gas does not react with water and that it is not appreciably soluble in it. These assumptions are valid for oxygen gas, but not for gases... [Pg.176]

FIGURE 21.2 Apparatus for the laboratary preparation of hydrogen gas. The gas is collected over water, as is also the case af oxygen gas (see Figure 5.13j. [Pg.833]

EXAMPLE 15 (fl) A mixture of oxygen and water vapor at a total pressure of 107 kPa is in equilibrium with liquid water at 25°C, at which temperature the water vapor pressure is 3.2 kPa. Calculate the pressure of the oxygen, (b) Oxygen is collected over water at 25°C under a barometric pressure of 107 kPa. (PH2O = 3.2 kPa) Calculate the pressure of the oxygen. [Pg.95]

In Figure 13.8 oxygen gas is being collected over water. Assume this experiment is being done at 25 °C. Write an equation for it, and find the pressure of the oxygen gas (assume the pressure in the bottle is Pj). [Pg.473]

Problem 5.55. A 2.5-L sample of oxygen was collected over water at 25 °C, and a total pressure of 745 torr. How many grams of oxygen were present ... [Pg.118]

The oxygen gas can be collected over water, as shown in Figure 5.15. Initially, the when collecting a gas over water, the total... [Pg.199]

When working stoichiometry problems like the one in the preceding section involving the decomposition of potassium chlorate, the oxygen is normally collected over water by displacement and the volume is then measured. However, in order to get the pressure of just the oxygen, you have to subtract the pressure due to the water vapor. You have to mathematically dry out the gas. [Pg.226]

Suppose, for example, that a sample of oxygen is collected over water at a total pressure of 755 torr at 20 degrees Celsius. And suppose that your job, you lucky dawg, is to calculate the pressure of the oxygen. [Pg.226]

How many grams of hydrogen are collected in a reaction where 1.78 L of hydrogen gas is collected over water at a temperature of 40 °C and a total pressure of 748 torr 108. How many grams of oxygen are collected in a reaction where 235 mL of oxygen gas is collected over water at a temperature of 25 °C and a total pressure of 697 torr ... [Pg.405]

All of the sodium peroxide reacted, and the oxygen was collected over water at 21°C. The barometric pressure was 771 mmHg. The apparatus was similar to that shown in Figure 5.20. However, the level of water inside the tube was 25.0 cm above the level of water outside the tube. If the volume of gas in the tube is 31.0 mL, how many grams of sodium peroxide were in the sample ... [Pg.223]

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