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2 years ago

The elements least likely to form bonds are found in which group?

Chemistry

1 answer:

taurus [48]2 years ago

4 0

Answer:

Noble gases are a unique set of elements in the periodic table because they don't naturally bond with other elements.

Explanation:

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From standard reduction potentials, calculate the equilibrium constant at 25 ∘c for the reaction 2mno−4(aq)+10cl−(aq)+16h+(aq)→2

garik1379 [7]

Answer:

$\boxed{\text{57.9}}$

Explanation:

Step 1. Determine the cell potential

E°/V

2MnO₄⁻ + 16H⁺ + 10e⁻ → 2Mn²⁺+ 8H₂O 1.507

10Cl⁻ ⟶ 5Cl₂ + 10e⁻ -1.358 27

2MnO₄⁻ + 10Cl⁻ + 16H⁺⟶ 2Mn²⁺ + 5Cl₂ + 8H₂O 0.149

Step 2. Calculate K

The formula relating K and E is

$E = \dfrac{RT}{nF} \ln K$

E = 0.149 V

R = 8.314 J·K⁻¹mol⁻¹

T = 25 °C = 298.15 K

n = 10

F = 96 485 C/mol

$0.149 = \dfrac{8.314 \times 298.15}{10\times 96 485} \ln K\\\\0.149 = 0.002 570 \ln K\\\\\ln K = \dfrac{0.149}{0.002570} = \textbf{57.9}$

The value of the equilibrium constant is $\boxed{\textbf{57.9}}$

6 0

2 years ago

if lithium loses an electron to become li+ what is the average atomic mass of the lithium ion? explain how you arrived at your a

Pavlova-9 [17]

The mass of an electron 1/1823 amu's = 0.0005 amu's... the average mass of litium is 6.941 amu's. by losing an electron, the mass of average atomic mass of the Lithium doesn't really change much.

8 0

3 years ago

Read 2 more answers

If you start with 163 g of water at 29◦C, how much heat must you add to convert all the liquid into vapor at 100◦C? Assume no he

Snowcat [4.5K]

Answer:

48.37514 kj

Explanation:

Given data:

Mass of water = 163 g

Initial temperature = 29°C

Final temperature = 100°C

Heat added = ?

Solution:

Specific heat capacity:

It is the amount of heat required to raise the temperature of one gram of substance by one degree.

Specific heat capacity of water is 4.18 j/g.°C

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = Final temperature - initial temperature

ΔT = 100°C - 29°C

ΔT = 71°C

Q = 163 g × 4.18 j/g.°C × 71°C

Q = 48375.14 j

Joule to Kj conversion:

48375.14 /1000 = 48.37514 kj

3 0

3 years ago

At 1023 K and 1 atm, a 3.00 gram sample of Snoz(s) (gram-formula mass = 151 g/mol) reacts with hydrogen gas to produce tin and w

Blizzard [7]

Answer:

2 moles of Sn are produced when 4 moles of H2(g) are consumed completely

Explanation:

to determine the number of moles of sn (l) produced when 4.0 moles of H2 (g) is consumed completely.

First, find the number of moles of H2 consumed by taking this as limiting reagent.

$n = \frac{g}{M.W (g/mol)}$

Then find the moles of Sn (l) taking into account the stoichiometric relationship between H2(g) and Sn(l). 2:1

$SnO_{2}$ (s) + 2 $H_{2}$ (g) ⇒ Sn(l) + 2 $H_{2}O$ (g)

$mol Sn(l) = \frac{1mol Sn}{2mol H_{2} } . 4 mol H_{2} = 2 mol$

∴2 moles of Sn are produced when 4 moles of H2(g) are consumed completely.

4 0

2 years ago

Can sombody pls help me with this

luda_lava [24]

Wouldn’t it be half of each? For 36 I guess is 18 and 54 will be 27, (NOT SURE)

6 0

2 years ago