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nataly862011 [7]
3 years ago
13

A potassium iodide compound is represented by which formula?

Chemistry
2 answers:
andrew11 [14]3 years ago
7 0
It is represented by C) KI

K+
I-

So it's KI
Tanya [424]3 years ago
5 0
<h2>Answer : Option C) KI</h2><h3>Explanation :</h3>

A potassium iodide compound is represented as KI.

It has K^{+} and I^{-} in it.

The potassium (K) reacts with Iodine vapors (I) to form KI (Potassium iodide).

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Write a balanced chemical equation for this reaction by completing the reaction below. Add the missing products and coefficients
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2 years ago
None of the given molecules display much solubility in water at room temperature. However, two of the molecules display apprecia
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5 0
2 years ago
PLSSSSS HELP I DONT GET THIS PROBLEMMMM
Aleks [24]

Answer:

C. 7370 joules.

Explanation:

There is a mistake in the statement. Correct form is described below:

<em>Using the above data table and graph, calculate the total energy in Joules required to raise the temperature of 15 grams of ice at -5.00 °C to water at 35 °C. </em>

The total energy needed to raise the temperature is the combination of latent and sensible heats, all measured in joules, and represented by the following model:

Q = m\cdot [c_{i} \cdot (T_{2}-T_{1})+L_{f} + c_{w}\cdot (T_{3}-T_{2})] (1)

Where:

m - Mass of the sample, in grams.

c_{i} - Specific heat of ice, in joules per gram-degree Celsius.

c_{w} - Specific heat of water, in joules per gram-degree Celsius.

L_{f} - Latent heat of fusion, in joules per gram.

T_{1} - Initial temperature of the sample, in degrees Celsius.

T_{2} - Melting point of water, in degrees Celsius.

T_{3} - Final temperature of water, in degrees Celsius.

Q - Total energy, in joules.

If we know that m = 15\,g, c_{i} = 2.06\,\frac{J}{g\cdot ^{\circ}C}, c_{w} = 4.184\,\frac{J}{g\cdot ^{\circ}C}, L_{f} = 334.72\,\frac{J}{g}, T_{1} = -5\,^{\circ}C, T_{2} = 0\,^{\circ}C and T_{3} = 35\,^{\circ}C, then the final energy to raise the temperature of the sample is:

Q = (15\,g)\cdot \left[\left(2.06\,\frac{J}{g\cdot ^{\circ}C} \right)\cdot (5\,^{\circ}C)+ 334.72\,\frac{J}{g} + \left(4.184\,\frac{J}{g\cdot ^{\circ}C}\right)\cdot (35\,^{\circ}C) \right]

Q = 7371.9\,J

Hence, the correct answer is C.

8 0
2 years ago
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