M HW Ch5c -> C Dezto.mheducation.com/hm.tpx e Chemistry question ! Chec × Questi

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M HW Ch5c -> C Dezto.mheducation.com/hm.tpx e Chemistry question ! Chec × Question 2 (of 3) Save & Exit Submit Save & Exit submit value 20.00 points 1 out of 2 attempts Enter vour answer in the provided box Assistance Check My Work View Hint View Question Show Me Guided Solution Question Help Report a Problem Aluminum reacts with excess hydrochloric acid to form aqueous aluminum chloride and 34.7 mL of hydrogen gas over water at 27°C and 751 mmHg. How many grams of aluminum reacted? The partial pressure of water at 27°C is 26.8 mmHg g Al 10:58 PM 3/7/2016 ·1111( ENG

Explanation / Answer

first find out the no of moles of H2 using PV = nRT formu

where P =751 mmHg convert in to atm = 1atm

V = 34.7 mL convert in to L = 0.0347 L

R = gas constant = 0.0821 Latm/mol-K

T = 27C = 27+273 = 300 K

put all these in the above equation

0.0347 x 1 = n x 0.0821 x 300K

n = 0.0347 / 24.63

n = 0.0014 moles

balanced equation is

2 Al + 6 HCl ----> 2 AlCl3 + 3 H2(g)

from this balanced equation it is clear that

2 moles of Al will give 3 moles of H2

howmany moles will give 0.0014 moles of H2

= 2 x 0.0014 / 3

= 9.4 x 10-4 moles

now we know the moles and molar mass we can take from text book ( 26.98 gram/mole)

weight of Al = moles of Al x molar mass of Al

weight = 0.00094 moles x 26.98 moles/grams

= 0.0253 grams

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