A sample of gas has a volume of 16.0 liters at a pressure of 0.5 atmospheres. When the volume decreases to 4.0 liters at a constant temperature, what will be the resulting pressure of the sample?

2 atm

Explanation:

From the question given above, the following data were obtained:

Initial volume (V₁) = 16.0 L

Initial pressure (P₁) = 0.5 atm

Final volume (₂) = 4 L

Final pressure (P₂) =?

The final pressure of the gas can be obtained by using the Boyle's law equation as illustrated below:

P₁V₁ = P₂V₂

0.5 × 16 = P₂ × 4

8 = P₂ × 4

Divide both side by 4

P₂ = 8 / 4

P₂ = 2 atm

Thus, the final pressure of the gas is 2 atm

i do not get it   at all

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2