Question

The following reaction is done at

T = 25°C and P= 1.0 atm:

Ca (s) + 2 HCl (aq) → CaCl_2 (aq) + H_2 (g)

If 500.0 g of calcium are added to an excess of HCI, what volume of H_2 is produced?​

Answer 1

Answer : The volume of
`H_` gas produced is, 305.8 L

Explanation :

First we have to calculate the moles of Ca.

`\text{Moles of Ca}=\frac{\text{Mass of Ca}}{\text{Molar mass of Ca}}`

Molar mass of Ca = 40 g/mol

`\text{Moles of Ca}=(500.0g)/(40g/mol)=12.5mol`

Now we have to calculate the moles of
`H_2` gas.

The balanced chemical reaction is:

`Ca(s)+2HCl(aq)\rightarrow CaCl_2(aq)+H_2(g)`

From the balanced chemical reaction we conclude that,

As, 1 mole of Ca react to give 1 mole of
`H_2` gas

So, 12.5 mole of Ca react to give 12.5 mole of
`H_2` gas

Now we have to calculate the volume of
`H_` gas.

Using ideal gas equation:

`PV=nRT`

where,

P = Pressure of
`H_2` gas = 1.0 atm

V = Volume of
`H_2` gas = ?

n = number of moles
`H_2` = 12.5 mole

R = Gas constant =
`0.0821L.atm/mol.K`

T = Temperature of
`H_2` gas =
`25^oC=273+25=298K`

Putting values in above equation, we get:

`1.0atm* V=12.5mole* (0.0821L.atm/mol.K)* 298K`

`V=305.8L`

Thus, the volume of
`H_` gas produced is, 305.8 L

Answer 2

Answer: 280dm3

Explanation:Please see attachment for explanation