If the reaction produces four8.0 l of h2 gas at a pressure of 0.995 atm and 32 degC, how many grams of cah2 are needed? This question is easy to answer if you know a bit about chemical equilibrium. The equation is straightforward: l = 0.9995 atm * 32 degC. The temperature is also an important factor in determining the amount of cah2 needed.
l of h2 gas at a pressure of 0.995 atm and a temperature of 32 degC
Calcium hydride is a chemical compound that reacts with water to form hydrogen gas. This chemical compound can also react with sulfuric acid, zinc, or aqueous sulfuric acid to form hydrogen gas. Using the ideal gas law, we can calculate the amount of hydrogen gas produced from these compounds. For example, a helium balloon has a volume of 5 poin 36.2 lat 300 k, so to generate 48.0 l of h2 gas we need to add 48.0 grams of calcium hydride and 0.8 atm of pressure.
The reaction between cah2 and H2 gas is highly complex, but a simple decomposition is not possible at 22oC. For that reaction to occur, the CaH2 must be heated to 1000oC and the temperature should be 32°C. During this reaction, the temperature of the two compounds is the same, but the rate of reaction is different.
gram of cah2
A sample of gas is in a flask at a temperature of 21 degC and a pressure of 697 mm Hg. A different gas is added to the flask, changing the temperature and pressure to 26 degC and 841 mm Hg. The unknown gas occupies 0.333 g of volume at standard pressure and 373 K. The unknown gas has a volume of 0.255 L and no known identity.
Given a sample of a gas at 21 degC and 697 mm Hg, what is the pressure and temperature required to produce an equal volume of the same gas at 26 degC and 841 mmHg? The unknown gas occupies a volume of 0.255 L at 373 K, and its identity is unknown. The reaction is called a reduction reaction, and the equilibrium constants are constants of the rate of reduction.