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zvonat [6]
4 years ago
5

Complete and balance the following redox equation using the set of smallest whole-number coefficients. Now sum the coefficients

of all species in the balanced equation. (Remember the coefficients that are equal to one.) BrO3-(aq) + Sb3+(aq) ? Br-(aq) + Sb5+(aq) (acid solution) The sum of the coefficients is ___.
Chemistry
1 answer:
EleoNora [17]4 years ago
4 0

Answer:

17

Explanation:

Oxidation reaction is defined as the chemical reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.

X\rightarrow X^{n+}+ne^-

Reduction reaction is defined as the chemical reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

X^{n+}+ne^-\rightarrow X

For the given chemical reaction:

BrO_3^-(s)+Sb^{3+}(aq.)\rightarrow Br^-(aq.)+5Sb^{5+}(aq)

The half cell reactions for the above reaction follows:

Reduction half reaction:  BrO_3^-+6H^++6e^-\rightarrow Br^{-}+3H_2O

Oxidation half reaction:  Sb^{3+}\rightarrow Sb^{5+}+2e^-

Multiplying the Oxidation half reaction by 3 and we get that:-

3Sb^{3+}\rightarrow 3Sb^{5+}+6e^-

Adding the half reactions, we get that:-

BrO_3^-+6H^++3Sb^{3+}\rightarrow Br^{-}+3Sb^{5+}+3H_2O

<u>The sum of the coefficients is:- 1 + 6 + 3 + 1 + 3 + 3 = 17</u>

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Explanation:

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3 0
3 years ago
The partial pressure of N2 in a mixture of gases, where the total pressure is 1.50 atm, is 300. torr. What is the mole fraction
makvit [3.9K]

Answer:

The mole fraction of N₂ is 0.26.

Explanation:

The pressure exerted by a particular gas in a mixture is known as its partial pressure. So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone:

PT = PA + PB

This relationship is due to the assumption that there are no attractive forces between the gases.

Dalton's partial pressure law can also be expressed in terms of the mole fraction of the gas in the mixture. The mole fraction is a dimensionless quantity that expresses the ratio of the number of moles of a component to the number of moles of all the components present.

So in a mixture of two or more gases, the partial pressure of gas A can be expressed as:

PA = XA * PT

In this case:

  • PA= PN₂= 300 torr
  • XA=XN₂= ?
  • PT= 1.50 atm= 1140 torr (being 1 atm= 760 torr)

Replacing:

300 torr= XN₂*1140 torr

Solving:

X_{N_{2} } =\frac{300 torr}{1140 torr}

XN₂= 0.26

<u><em>The mole fraction of N₂ is 0.26.</em></u>

6 0
3 years ago
A sample of He at 25C and 755 torr occupies a fixed volume of 16.8L. What mass of He must be pumped in to increase the pressure
AURORKA [14]

Answer:

2.4 g

Explanation:

Step 1: Given data

  • Initial pressure (P₁): 755 torr
  • Volume (V): 16.8 L
  • Temperature (T): 25 °C
  • Final pressure (P₂): 1.87 atm

Step 2: Convert "P₁" to atm

We will use the conversion factor 1 atm = 760 torr.

755 torr × 1 atm/760 torr = 0.993 atm

Step 3: Convert "T" to K

We will use the following expression.

K = °C + 273.15

K = 25°C + 273.15 = 298 K

Step 4: Calculate the initial number of moles of He

We will use the ideal gas equation.

P₁ × V = n₁ × R × T

n₁ = P₁ × V/R × T

n₁ = 0.993 atm × 16.8 L/(0.0821 atm.L/mol.K) × 298 K

n₁ = 0.682 mol

Step 5: Calculate the final number of moles of He

We will use the ideal gas equation.

P₂ × V = n₂ × R × T

n₂ = P₂ × V/R × T

n₂ = 1.87 atm × 16.8 L/(0.0821 atm.L/mol.K) × 298 K

n₂ = 1.28 mol

Step 6: Calculate the moles of He added

n = n₂ - n₁

n = 1.28 mol - 0.682 mol

n = 0.60 mol

Step 7: Convert "n" to mass

The molar mass of He is 4.00 g/mol

0.60 mol × 4.00 g/mol = 2.4 g

8 0
3 years ago
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