What is the mass of hydrogen in 5.5 mol of Ca(OH)2?

Chemistry

1 answer:

Morgarella [4.7K]3 years ago

3 0

Answer:

12*2*6.022*10^23. Atoms of hydrogen.

Explanation:

First of all if u know that 1 molecule of calcium hydroxide contain 2 hydrogen atom and 1 mole of calcium hydroxide contain 6.022*10^23 molecules of calcium hydroxide.

Hence 1 mole of calcium hydroxide contain 2*6.022*10^23 atom of hydrogen.

So 12 mole of calcium hydroxide contain =12*2*6.022*10^23. Atoms of hydrogen.

You might be interested in

A sample of oxygen gas has a volume of 36.7 L at 145 kPa and 65. ̊C. What volume will the sample have at STP?

xxTIMURxx [149]

Data Given:

Initial Volume = V₁ = 36.7 L

Initial Pressure = P₁ = 145 kPa

Initial Temperature = T₁ = 65 °C + 273 = 338 K

Final Volume = V₂ = ?

Final Pressure = P₂ = 101.325 kPa (Standard Pressure)

Final Temperature = T₂ = 273 K (Standard Temperature)

Formula used:
As number of moles are constant, so Ideal Gas equation in following form is used,
P₁ V₁ / T₁ = P₂ V₂ / T₂
Solving for V₂,
V₂ = P₁ V₁ T₂ / T₁ P₂
Putting Values,

V₂ = (145 kPa × 36.7 L × 338 K) ÷ (273 K × 101.325 kPa)

V₂ = 1798667 ÷ 27661.25

V₂ = 65.02 L

8 0

3 years ago

Most of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas well

galben [10]

Answer:

$0.21\ \text{kg/s}$

Explanation:

P = Pressure = $0.48\ \text{atm}=0.48\times 101325\ \text{Pa}$

V = Volume = $450\ \text{L/s}=450\times 10^{-3}\ \text{m}^3/\text{s}$

R = Gas constant = $8.314\ \text{J/mol K}$

T = Temperature = $(264+273.15)\ \text{K}$

The reaction is

$2H_2S+3O_2\rightarrow 2SO_2+2H_2O$

From ideal gas equation we have

$PV=nRT\\\Rightarrow n=\dfrac{PV}{RT}\\\Rightarrow n=\dfrac{0.48\times101325\times 450\times 10^{-3}}{8.314\times (264+273.15)}\\\Rightarrow n=4.9\ \text{mol}$