Calcium hydride (cah2) reacts with water to form hydrogen gas: cah2(s) + 2h2o(l) → ca(oh)2(aq) + 2h2(g)how many grams of cah2 are needed to generate 48.0 l of h2 gas at a pressure of 0.888 atm and a temperature of 32°c? calcium hydride (cah2) reacts with water to form hydrogen gas: cah2(s) + 2h2o(l) → ca(oh)2(aq) + 2h2(g)how many grams of cah2 are needed to generate 48.0 l of h2 gas at a pressure of 0.888 atm and a temperature of 32°c? 35.850.70.85171.7143

The mass of calcium hydride needed is 35.8 grams

Explanation:

To calculate the moles of hydrogen gas, we use the equation given by ideal gas, which follows:

where,

P = pressure of the hydrogen gas = 0.888 atm

V = Volume of the hydrogen gas = 48.0 L

T = Temperature of the hydrogen gas =

R = Gas constant =

n = number of moles of the hydrogen gas = ?

Putting values in above equation, we get:

The given chemical equation follows:

By Stoichiometry of the reaction:

2 moles of hydrogen gas is produced by 1 mole of calcium hydride

So, 1.702 moles of hydrogen gas will be produced from = of calcium hydride

Now, calculating the mass of calcium hydride by using the equation:

Moles of calcium hydride = 0.851 moles

Molar mass of calcium hydride = 42 g/mol

Putting values in above equation, we get:

Hence, the mass of calcium hydride needed is 35.8 grams