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IRISSAK [1]
3 years ago
14

The following balanced equation shows the formation of water.

Chemistry
2 answers:
ss7ja [257]3 years ago
8 0
Mole ratio of H₂  :  O₂   is   2  :  1

∴ if mole of H₂  =  1.67 mol

then mole of O₂ =  \frac{1.67   mol}{2}

⇒ that mole of oxygen needed to react with H₂  =  0.835 mol

The answer is A
saveliy_v [14]3 years ago
8 0

Answer: A) 0.835 mol of O_2

Explanation: According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

As can be seen from the given balanced equation:

2H_2+O_2\rightarrow 2H_2O

2 moles of hydrogen are required to react completely with 1 mole of oxygen.

Thus 1.67 moles of hydrogen will react with=\frac{1}{2}\times 1.67=0.835 moles of oxygen.

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the relative molecular mass of hydrated iron (II) sulfate FeSO4.7H2O is 278.02

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Hat is used and produced in glycoloysis?
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<h3>What is glycolysis?</h3>

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2 years ago
Calculate the energy (in kJ) required to heat 10.1 g of liquid water from 55 oC to 100 oC and change it to steam at 100 oC. The
Maksim231197 [3]

Answer:

           \large\boxed{\large\boxed{24.6kJ}}

Explanation:

<u>1. Energy to heat the liquid water from 55ºC to 100ºC</u>

     Q=m\times C\times \Delta T

  • m = 10.1g
  • C = 4.18g/JºC
  • ΔT = 100ºC - 55ºC = 45ºC

     Q=10.1g\times 4.18J/g\ºC\times 45\ºC=1,899.81J

<u>2. Energy to change the liquid to steam at 100ºC</u>

      L=\lambda \times n

  • λ = 40.6kJ/mol
  • n = 10.1g / 18.015g/mol = 0.5606mol

      L=40.6kJ/mol\times 0.5604mol=22.76214kJ=22,762.14J

<u>3. Total energy</u>

       1,899.81J+22,762.14J=24,661.95J\approx24,662J\approx24.6kJ

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See the image below-⬇⬇-

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