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2 years ago

What is the bond energy per mole for breaking all the bonds of oxygen, O 2 ?

1 answer:

4 0

There is only one O=O bond in an O2 molecule, so the energy ΔHO2 required for breakingall the bonds in a mole of O2 molecules is 498 kJ/mol O2 molecules. Calculate the bond energy per mole for forming all the bonds of water molecules, H2O

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During a lab experiment performed at STP conditions, you prepare HCl by reacting 100. ml of Cl2 gas with an excess of H2 gas.

Brrunno [24]

Answer: 19.4 mL Ba(OH)2

Explanation:

H2(g) + Cl2(g) --> 2HCl(aq) (make sure this equation is balanced first)

At STP, 1 mol gas = 22.4 L gas. Use this conversion factor to convert the 100. mL of Cl2 to moles.

0.100 L Cl2 • (1 mol / 22.4 L) = 0.00446 mol Cl2

Use the mole ratio of 2 mol HCl for every 1 mol Cl2 to find moles of HCl produced.

0.00446 mol Cl2 • (2 mol HCl / 1 mol Cl2) = 0.00892 mol HCl

HCl is a strong acid and Ba(OH)2 is a strong base so both will completely ionize to release H+ and OH- respectively. You need 0.00892 mol OH- to neutralize all of the HCl. Note that one mole of Ba(OH)2 contains 2 moles of OH-.

0.00892 mol OH- • (1 mol Ba(OH)2 / 2 mol OH-) • (1 L Ba(OH)2 / 0.230 M Ba(OH)2) = 0.0194 L = 19.4 mL Ba(OH)2

3 0

2 years ago

5.00 g of hydrogen gas and 50.0g of oxygen gas are introduced into an otherwise empty 9.00L steel cylinder, and the hydrogen is

GenaCL600 [577]

1) Balanced chemical reaction:

2H2 + O2 -> 2H20

Sotoichiometry: 2 moles H2: 1 mol O2 : 2 moles H2O

2) Reactant quantities converted to moles

H2: 5.00 g / 2 g/mol = 2.5 mol

O2: 50.0 g / 32 g/mol = 1.5625 mol

Limitant reactant: H2 (because as per the stoichiometry it will be consumed with 1.25 mol of O2).

3) Products

H2 totally consumed -> 0 mol at the end

O2 = 1.25 mol consumed -> 1.5625 mol - 1.25 mol = 0.3125 mol at the end

H2O: 2.5 mol H2 produces 2.5 mol H2O -> 2.5 mol at the end.

Total number of moles: 0.3125mol + 2.5 mol = 2.8125 mol

4) Pressure

Use pV = nRT
n = 2.8125
V= 9 liters
R = 0.082 atm*lit/K*mol
T = 35 C + 273.15 = 308.15K

p = nRT/V = 7.9 atm

3 0

2 years ago

Read 2 more answers

For lunch, a patient consumed 3 oz of skinless chicken, 3 oz of broccoli, 1 medium apple, and 1 cup of nonfat milk (see Table 3.

Volgvan

Lunch of a patient has 3 oz skinless chicken, 3 oz of broccoli, 1 medium apple, and 1 cup of nonfat milk

Energy content of 3 oz skinless chicken is = 110 kcal

Energy content of 3 oz broccoli = 30 kcal

Energy content of 1 medium apple = 60 kcal

Energy content of 1 cup non-fat milk = 90 kcal

So the kilocalories of energy patient obtained from lunch

= 110 kcal+ 30 kcal + 60 kcal + 90 kcal = 290 kcal

3 0

2 years ago

Consider the decomposition of the compound C5H6O3 as follows below. C5H6O3(g) → C2H6(g) + 3 CO(g) When a 5.63-g sample of pure C

timofeeve [1]

Answer:

K = 6.5 × 10⁻⁶

Explanation:

C₅H₆O₃ ⇄ C₂H₆ + 3CO

Use PV=nRT to find the initial pressure of C₅H₆O₃

P (2.50) = (0.0493) (0.08206) (473)

P = 0.78atm

C₅H₆O₃ ⇄ C₂H₆ + 3CO

0.78atm 0 0

0.78 - x x 3x

1.63atm = 0.78 - x + x + 3x

P(total) = 0.288atm

C₅H₆O₃ = 0.78 - 0.288

= 0.489atm

C₂H₆ = 0.288atm

CO = 0.846atm

$K_p = \frac{0.288 * 0.864^3}{0.489}$

= 0.379

$K = \frac{K_p}{RT^3}$

$K = \frac{0.379}{(0.0821 * 473)^3}$

= 6.5 × 10⁻⁶

7 0

2 years ago

A student creates a mixture of water and washing soda weighing 10 g and a mixture of

Anni [7]

Answer: The weight of the products should be the same after he mixes them.

Explanation: The law of the conservation of mass states that the mass of the products in a chemical reaction must equal the mass of the reactants. Even if the products are changed or rearranged, the products and reactants will still have the same mass

8 0

2 years ago