Chemistry, asked by subhashreepraharaj19, 15 hours ago

Solid aluminum reacts with aqueous H2SO, to form H, gas
and aluminum sulfate. When a sample of Al is allowed to
react, 415 mL of gas is collected over water at 23 °C, at
a pressure of 755 mmHg. At 23 °C. the vapor pressure of
water is 21 mmHg. (11.7, 118, 11.9)
3H,SO,(aq) + 2Al(s) 3H2(g) + Al-(S0.),(aq)
a. What is the pressure, in millimeters of mercury, of the
dry Hgas?
b. How many moles of H, were produced?
c. How many grams of Al were reacted?

Answers

Answered by nagendragoswami4
0

Answer:

2Al+3H

2

SO

4

→Al

2

(SO

4

)

3

+3H

2

27

5.7

1000

50×5

=0.2mole =0.25 mole (Limiting reagent)

∴0.25 mole H

2

is formed

PV=nRT

V=

P

nRT

=

1atm

0.25×0.082×300

V=6.15 litre

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