A sample of ideal gas has a volume of 0.500-L at 25.0o C and 1.20 atm pressure. What is the volume at 75.0o C and 3.60 atm?

.500

Explanation:

Use the ideal gas law equation: PV = nRT

Plug in the initial values given:

P = 1.2 atm

V = .500 L

n = number of moles

R = Gas Constant 8.314

T = 25.0 C

(1.2)(.5) = n(8.314)(25)

solving for n we get .00289

Now use the same equation with the new values solving for V

(3.6)V = (.00289)(8.314)(75.0)

V = .4999999 ROund to .500

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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