Calculating gas volumes

What mass of magnesium oxide is formed by burning 1.2 g of magnesium metal in oxygen  

When gases are involved in reactions, it is easier to measure their volumes rather than weigh them and find their masses. Although we can calculate the masses of gases used up or produced in chemical reactions using the methods described in the previous section, it is often more convenient to calculate the volumes involved. 

One mole of ANY gas occupies a volume of 24 dm at room temperature and pressure. 

Work out the mole relationship between the substances you are considering  

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Finally, to eliminate the effect of prospect area on the calculations, gas volumes are essentially normalized by computing the volumes in... 

The most important use of the real gas law is to calculate the volume which a subsurface quantity of gas will occupy at surface conditions, since when gas sales contracts are negotiated and gas is subsequently sold it is referred to in volumes at standard conditions of temperature (Tsc) and pressure (Psc). 

Adamczyk (1976) is one of the few who tried to incorporate energy losses from the irreversible shock process into the calculation. He proposes to use the work done by gas volume in a process illustrated in Figure 6.12 and described below. 

Gas volumes are corrected at the intake conditions on the first and each succeeding stage of the compression step, and compressibility factors are calculated or evaluated at these individual intake conditions. Some manufacturers use the average value between intake and discharge conditions. 

Again, use the ideal gas law to find the mass of water that must be vaporized to reach the calculated pressure (7.9 mm Hg). Subtract the mass of vaporized water from the mass of water in the vaporizer, and use density to calculate the volume of water in the vaporizer. 

Strategy First (1), write a balanced equation for the reaction, which is very similar to that for ZnS, except that Zn2+ is replaced by Bi3+. (2) Using the balanced equation, calculate the number of moles of S02. Finally (3), use the ideal gas law to calculate the volume of S02. 

Step I. We must convert the specified volume of S02 into moles. A convenient way to do this is to calculate the volume this gas would occupy under conditions at which we know the volume occupied by one mole of gas. For example, we know that one mole of gas occupies 22.4 liters at 0°C and one atmosphere pressure. Increasing the temperature of a gas at constant... 

When making calculations, we will generally convert all data to their values in SI units, since calculations involving SI units give answers in SI units. For example, when calculating the volume of an ideal gas from the equation... 

Table 4.3 gives values of the molar volume of an ideal gas under a variety of common conditions. To obtain the volume of a known amount of gas at a specified temperature and pressure, we simply multiply the molar volume at that temperature and pressure by the amount in moles. Alternatively, we can use the ideal gas law to calculate the volume. 

The apparent reaction rate constant for the first order reaction, k, was calculated from the conversion of CO2. Since the gas-volume reduction rate increased with k, a poor fluidization was induced by high reaction rate. We investigated the effect of the rate of the gas-volume change on the fluidization quality. The rate of the gas-volume change can be defined as rc=EA(dxA/dt), where Sa is the increase in the number of moles when the reactants completely react per the initial number of moles. This parameter is given by 7-1. When the parameter, Ea, is negative, the gas volume decreases as the reaction proceeds. 

C21-0095. A company that manufactures photographic film generates 2550 L/day of aqueous waste containing 0.125 g/L of Br ions. To recover the bromine in the form of Bf2, the company bubbles CI2 gas through this waste. Calculate the volume of gas that is consumed daily if the gas is delivered at 1.05 atm and 21 °C. 

The comparison of experimental data on determination of concentrations of H- and O-atoms in the gas volume or on the surface using semiconductor ZnO films given in this Section with results of calculations based on the formulas derived in Chapter 2 we can conclude that even extremely small concentrations of active particles (10 to 10 m ) can be assessed quantitatively by sensors both in the gaseous phase and on the surface of solid bodies (see below). 

The vessel is determined to be an uninsulated, horizontal, grade-level, cylindrical pressure vessel with a gas volume of 706 ft3 (20 m3). The vessel has a MAWP of 1,480 psig (102 bar) at 650°F (343°C) and a Minimum Design Metal Temperature (MDMT) of 40°F (4°C) since it is constructed of unnormalized steel material. Due to process conditions immediately prior to pressuring the vessel to 1,000 psig (69 bar), the vessel s metal temperature is approximately 30°F (-1°C). When the vessel is pressurized to 1,000 psig, it fails catastrophically. The distances to overpressure endpoints (1, 3, and 5 psig) are calculated as follows ... 

Plan (1) Use the Combined Gas Law to calculate the volume that 1 L of the gas would have occupied... 

Calculate the volume of hydrogen gas, measured at room temperature and pressure, which would be formed when 12 g of magnesium react with excess dilute sulphuric acid (assume that one mole of any gas occupies a volume of 24,000 cm3 (24 dm3) at room temperature and pressure relative atomic mass of... 

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