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deff fn [24]
3 years ago
9

Which ion will most likely form a precipitate when reacted with SO42 ?

Chemistry
1 answer:
Charra [1.4K]3 years ago
6 0
<h2>Answer:Ba^2+</h2>

Explanation:

option A:

SO_{4}^{2-} is an anion and Cl^{1-} is also an anion.So,there is no reaction.

option B:

K^{+} reacts with SO_{4}^{2-} to form K_{2}SO_{4}.

Since K is a first group element,all its salts are soluble in water.

Hence no precipitate is formed.

option C:

Na^{+} reacts with SO_{4}^{2-} to form Na_{2}SO_{4}.

Since Na is a first group element,all its salts are soluble in water.

Hence no precipitate is formed.

option D:

Ba^{2+} reacts with SO_{4}^{2-} to form BaSO_{4}.

Solubility of sulphates of second group elements decrease down the group.

So,BaSO_{4} is a precipitate.

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Which of earths spheres contains most of its mass?
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A nuclear reactor core must stay at or below 95 °C to remain in good working condition. Cool water at a temperature of 10 °C is
aliina [53]

Answer:

\large \boxed{\text{67 000 g}}

Explanation:

This is a problem in calorimetry — the measurement of the quantities of heat that flow from one object to another.

It is based on the Law of Conservation of Energy — Energy can be transformed from one type to another, but it cannot be destroyed or created.

If heat flows out of the reactor (negative), the same amount of heat must flow into the water (positive).

Since there is no change in total energy,

heat₁ + heat₂ = 0

The symbol for the quantity of heat transferred is q, so we can rewrite the word equation as

q₁ + q₂  = 0

The formula for the heat absorbed or released by an object is

 q = mCΔT, where

 m = the mass of the sample

  C = the specific heat capacity of the sample, and

ΔT = T_f - T_i = the change in temperature

1. Equation

There are two heat flows in this problem,

heat released by reactor + heat absorbed by water = 0

               q₁                  +                        q₂                     = 0

               q₁                  +                 m₂C₂ΔT₂                 = 0

2. Data:

q₁ = -23 746 kJ

m₂ = ?; C₂ = 4.184 J°C⁻¹g⁻¹;  T_f = 95 °C; T_i = 10 °C

3. Calculations

(a) Convert kilojoules to joules

q_{1} = -\text{23 746 kJ} \times \dfrac{\text{1000 J}}{\text{1 kJ}} = -\text{23 746 000 J}

(b) ΔT  

ΔT₂ = T_f - T_i = 95 °C - 10 °C = 85 °C

(c) m₂

\begin{array}{rcl}q_{1} + q_{2} & = & 0\\\text{-23 746 000 J} + m_{2} \times 4.184 \text{ J$^{\circ}$C$^{-1}$g$^{-1}$} \times 85 \, ^{\circ}\text{C} & = & 0\\\text{-23 746 000 J} + 356m_{2} \text{J$\cdot$g}^{-1} & = & 0\\356m_{2} \text{g}^{-1} & = & 23746000\\m_2&=& \dfrac{23746000}{\text{356 g}^{-1}}\\\\ & = & \textbf{67000 g}\\\end{array}\\

\text{You must circulate $\large \boxed{\textbf{67 000 g}}$ of water each hour.}

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Two examples of energy transformations are shown.
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The fire- chemical energy is turned to light energy during the combustion of carbon.  Both products comprise of ultraviolet radiation which is a form of radiant energy.

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