At a constant pressure, what temperature will be reached if a gas at 300 K with a volume of 0.1 liters is increased to 0.2 liters?

600K

Explanation:

The following were obtained from the question.

Initial temperature (T1) = 300K

Initial Volume (V1) = 0.1L

Final volume (V2) = 0.2L

Final temperature (T2) =?

Step 2:

Determination of the final temperature.

Since the pressure is constant, the gas is simply obeying Charles' law.

Using the Charles' law equation, the final temperature can be obtained as follow:

V1/T1 = V2 /T2

0.1/300 = 0.2/T2

Cross multiply to express in linear form

0.1 x T2 = 300 x 0.2

Divide both side by 0.1

T2 = (300 x 0.2)/0.1

T2 = 600K

i think slash and

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