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n200080 [17]
3 years ago
15

Which of these equations is balanced? a. 3 H2SO4 + 2Al → Al2(SO4)3 + 3H2 b. 2KCl + Pb(NO3)2 → KNO3 + PbCl2 a b a and b neither

Chemistry
2 answers:
wolverine [178]3 years ago
8 0
A.) 3 H2SO4 + 2 Al > Al2(SO4)3 + 3 H2
6 H+ +3 S +12 O +2 Al> 2 Al + 3S + 12O + 6H+
This one is balanced, with 6 H, 3 S, 12 O, and 2 Al on both sides.
B.) 2KCl + Pb(NO3)2 > KNO3 + PbCl2
2K + 2Cl + Pb + 2N +6 O > 1 K + 1 N+ 3 O + Pb + 2 Cl
This one is not balanced as there is 2 K, 6 O and 2 N on the reactants side but only 1 K, 3 O, and 1 N on the products side.
Therefore, only A.) is balanced
Nataly_w [17]3 years ago
3 0
Only equation A is balanced.
To balance equation B, simply add another molecule of KNO3, so the final equation would be:
2KCl + Pb(NO3)2 ---> 2KNO3 + PbCl2

Please mark my answer as brainliest
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Andre45 [30]

The increasing order of standard molar entropy (S°) is as follow:

SF₄(g) < SF₆(g) < S₂F₁₀(g)

<h3>What is Entropy? </h3>

Entropy is defined as the randomness of the particle. It depends on temperature and pressure or number of particle per unit volume.

It is directly proportional to the temperature and pressure of the gas.

<h3>What is Standard Molar Entropy? </h3>

The standard molar entropy is defined as the entropy content of the one mole of pure substance at the standard state of temperature and pressure of interest.

The standard molar entropy is also defined as the total amount of entropy which 1 mole of the substance acquire, as it is brought from 0K to standard conditions of temperature and pressure.

The standard molar entropy depends on the molas mass of atom, molecules or compound.

SF₄(g) has lower standard molar entropy. Due to less complexity of this molecules.

While, complexity increases from SF₆(g) to S₂F₁₀(g). Therefore, the standard molar entropy of S₂F₁₀(g) is greater than SF₆(g).

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1 year ago
The equilibrium constant for the reaction
Hitman42 [59]

The question is incomplete, here is the complete question:

The equilibrium constant for the reaction

N₂O₄(g)⇌2NO₂ at 2°C is Kc = 2.0

If each yellow sphere represents 1 mol of N₂O₄(g) and each gray sphere 1 mol of NO₂ which of the following 1.0 L containers represents the equilibrium mixture at 2°C?

The image is attached below.

<u>Answer:</u> The system which represents the equilibrium having value of K_c=2.0 is system (b)

<u>Explanation:</u>

Equilibrium constant in terms of concentration is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as K_c

For a general chemical reaction:

aA+bB\rightarrow cC+dD

The expression for K_{c} is written as:

K_{c}=\frac{[C]^c[D]^d}{[A]^a[B]^b}

For the given chemical equation:

N_2O_4(g)\rightleftharpoons 2NO_2

The expression of K_c for above equation follows:

K_c=\frac{[NO_2]^2}{[N_2O_4]}      .......(1)

We are given:

Volume of the container = 1.0 L

Value of K_c = 2.0

Molarity of the substance is calculated by using the equation:

\text{Molarity}=\frac{\text{Number of moles}}{\text{Volume}}

For the given images:

  • <u>For a:</u>

Number of Gray spheres = 8 moles

Number of yellow spheres = 4 moles

Putting values in expression 1, we get:

K_c=\frac{(8/1)^2}{(4/1)}\\\\K_c=16

  • <u>For b:</u>

Number of Gray spheres = 4 moles

Number of yellow spheres = 8 moles

Putting values in expression 1, we get:

K_c=\frac{(4/1)^2}{(8/1)}\\\\K_c=2

  • <u>For c:</u>

Number of Gray spheres = 6 moles

Number of yellow spheres = 6 moles

Putting values in expression 1, we get:

K_c=\frac{(6/1)^2}{(6/1)}\\\\K_c=6

  • <u>For d:</u>

Number of Gray spheres = 2 moles

Number of yellow spheres = 8 moles

Putting values in expression 1, we get:

K_c=\frac{(2/1)^2}{(8/1)}\\\\K_c=\frac{1}{2}

Hence, the system which represents the equilibrium having value of K_c=2.0 is system (b)

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cluponka [151]

Answer:

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WITCHER [35]
1) State the balanced chemical equation

Na3 PO4                  + 3 AgNO3        → 3NaNO3        +        Ag3 PO4

sodium phosphate        silver nitrate       sodium nitrate    silver phosphate

2) State the molar ratios

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3) As you see 3 moles of Silver Nitrate react with 1 mol of Na3 PO4, then you will need.

The you need to use the molar ratio 1:3 to calculate the number of moles of sodium phosphate

1 mol Ag NO3 * [ 1 mol Na3 PO4 / 3 mol Ag NO3] = 0.33 mol Na3 PO4

Answer: 0.33 mol sodium phosphate
3 0
3 years ago
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