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choli [55]
3 years ago
12

If 2.00 moles of H₂ and 1.55 moles of O₂ react how many moles of H₂O can be produced in the reaction below?

Chemistry
1 answer:
jekas [21]3 years ago
5 0

Answer:

2 mol H₂O

Explanation:

With the reaction,

  • 2H₂(g) + O₂(g) → 2 H₂O(g)

1.55 moles of O₂ would react completely with ( 2*1.55 ) 3.1 moles of H₂. There are not as many moles of H₂, thus H₂ is the limiting reactant.

Now we <u>calculate the moles of H₂O produced</u>, <em>starting from the moles of limiting reactant</em>:

  • 2.00 mol H₂  * \frac{2molH_2O}{2mol H_2} = 2 mol H₂O
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How many liters of hydrogen gas are formed from the complete reaction of 1.03 mol of C? Assume that the hydrogen gas is collecte
aliina [53]

Answer:

27 liters of hydrogen gas will be formed

Explanation:

Step 1: Data given

Number of moles C = 1.03 moles

Pressure H2 = 1.0 atm

Temperature = 319 K

Step 2: The balanced equation

C +H20 → CO + H2

Step 3: Calculate moles H2

For 1 mol C we need 1 mol H2O to produce 1 mol CO an 1 mol H2

For 1.03 moles C we'll have 1.03 moles H2

Step 4: Calculate volume H2

p*V = n*R*T

⇒with p = the pressure of the H2 gas = 1.0 atm

⇒with V = the volume of H2 gas = TO BE DETERMINED

⇒with n = the number of moles H2 gas = 1.03 moles

⇒with R = the gas constant = 0.08206 L*Atm/mol*K

⇒with T = the temperature = 319 K

V = (n*R*T)/p

V = (1.03 * 0.08206 *319) / 1

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