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Novay_Z [31]
3 years ago
11

Which of the following is true about a system at equilibrium? a The concentration(s) of the reactant(s) is equal to the concentr

ation(s) of the product(s). b No new product molecules are formed. c The concentration(s) of reactant(s) is constant over time. d The rate of the reverse reaction is equal to the rate of the forward reaction and both rates are equal to zero. e None of the above (a-d) is true.
Chemistry
1 answer:
anyanavicka [17]3 years ago
6 0

Answer:

c The concentration(s) of reactant(s) is constant over time.  

Step-by-step explanation:

When the reaction A ⇌ B reaches equilibrium, the concentrations of reactants and products are constant over time.

a is <em>wrong</em>, because the concentrations of reactants and products are usually quite different.

b is <em>wrong</em>, because both product and reactant molecules are being formed at equilibrium.

d is <em>wrong</em>. The rates of the forward and reverse reactions are equal, but they are not zero.

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How many protons and electrons are in Hg+
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Answer:

There are 80 protons and 80 electrons in Hg+ (Mercury)

Explanation:

Name Mercury

Symbol Hg

Atomic Number 80

Atomic Mass 200.59 atomic mass units

Number of Protons 80

Number of Neutrons 121

Number of Electrons 80

Melting Point -38.87° C

Boiling Point 356.58° C

Density 13.456 grams per cubic centimeter

Normal Phase Liquid

Family Transitions Metals

Period Number 6

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Ranging from 0 to 14, a pH value indicates how acidic or basic a solution is. Which of these pH values would be a strong acid? *
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Which of the following is a physical change?
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A rabbit has a mass of 2 kg. what is the weight?
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2 years ago
Determine the molarity of a 6.0 mole% sulfuric acid solution with SG-a 1.07 Note: Atomic Weight: S (32), O 16); H (O)
marin [14]

Answer:

The molarity of a 6.0 mole% sulfuric acid solution is 2.8157 Molar.

Explanation:

Suppose there are 100 moles in solution:

Moles of sulfuric acid = 6% of 100 moles = 6 moles

Mass of 6 moles of sulfuric acid = 6 mol × 98 g/mol=588 g

Moles of water = 100%- 6% = 94%= 94 moles

Mass of water = 94 mol × 18 g/mol = 1692 g

Specific gravity of the solution ,S.G= 1.07

Density of solution = D

S.G=\frac{D}{d_w}

d_w = density of water = 1 g/mL

D=S.G\times d_w=1.07\times 1 g/mL=1.07 g/mL

Mass of the solution = 588 g + 1692 g = 2280 g

Volume of the solution = V

Volume = \frac{Mass}{Density}

=\frac{2280 g}{1.07 g/mL}=2130.84 mL=2.13084 L

1 mL = 0.001 L

Molarity = \frac{n}{V(L)}

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V = 2.13084 L

So, the molarity of the solution is :

Molarity=\frac{6 mol}{2.13084 L}=2.8157 mol/L

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