Question

The following reaction is done at

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

$\text{Moles of Ca}=\frac{500.0g}{40g/mol}=12.5mol$

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:

$1.0atm\times V=12.5mole\times (0.0821L.atm/mol.K)\times 298K$

$V=305.8L$

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

Answer 2

Answer: 280dm3

Explanation:Please see attachment for explanation