Extra Practice Problem #2

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Hena Sihota 1L
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Joined: Fri Sep 29, 2017 7:07 am
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Extra Practice Problem #2

Postby Hena Sihota 1L » Thu Nov 09, 2017 2:34 pm

How would you solve this problem:
The following two-step reaction produces hydrogen.
Step 1: CH4+H2O->CO+3H2
Step 2: CO+H2O->CO2+H2
Given 0.036g of methane (CH4) and 0.108g of water, how much hydrogen, in grams, is produced?

Ishan Saha 1L
Posts: 60
Joined: Fri Sep 29, 2017 7:03 am

Re: Extra Practice Problem #2

Postby Ishan Saha 1L » Thu Nov 09, 2017 2:41 pm

Hi! I'm guessing that the second reaction uses H2O in excess? If so, then first you find the limiting reagent in the first reaction, and calculate the maximum amount of CO that can be produced while keeping the limiting reactant in mind. The product, CO, from the first reaction is used as a reactant in the second reaction. So calculate how many moles of H2 can be produced with CO as the limiting reactant (since you only have as much CO as was produced in the first reaction). Finally, convert moles of Hydrogen to grams.

Ishan Saha 1L
Posts: 60
Joined: Fri Sep 29, 2017 7:03 am

Re: Extra Practice Problem #2

Postby Ishan Saha 1L » Thu Nov 09, 2017 3:26 pm

Also to find the total hydrogen produced, you need to add the hydrogen produced in the first reaction to the hydrogen produced in the second reaction.


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