It is known that amu is equal to the molar mass of 1 mole of substance. Therefore,

Weight of one mole of uranium = 238 g/mol

The molar mass or molecular weight for U205 is 556 g/mol.
(238 x 2) + (16 x 5) = 556 g/mol

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4 years ago

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Draw the Lewis structure for the sulfur dioxide molecule. Be sure to include all resonance structures that satisfy the octet rul

trapecia [35]

Answer:

See explanation

Explanation:

We have to remember that the formula of sulfur dioxide is $SO_2$ . So, the "S" atom is the central one and the "O" atoms are in the left and right of S. Additionally, "S" and "O" atom has 6 valence electrons each. With this in mind, we can start with a structure in which the left oxygen has 2 lone pairs and a double bond, the S atom can have a double bond a single bond and a lone pair and the right oxygen with 3 lone pairs with a single bond (structure A). Now, if we move the negative charge in the right (resonance) to the middle and the double bond to the left oxygen we will obtain structure B. Finally, we can move the negative charge in the left to the middle and we will obtain structure C. (See figure 1).

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3 years ago

Balance the reaction. A coefficient of "1" is understood. Choose option "blank" for the correct answer if the coefficient is "1.

Ann [662]

2HCL + __ Zn --> ZnCl2 + H2

i think that's right, not exactly sure.

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4 years ago

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Wheen 56j of heat are added to 11g of liquid, its temperature rises from 10.4 degrees celsius to 12 degrees celsius. What is the

svetoff [14.1K]

$c = 3.2 \; \text{J} \cdot \text{kg}^{-1} \cdot \text{K}^{-1}$

Energy change $Q = 56 \; \text{J}$
Mass being heated $m = 11 \; \text{g}$
Temperature change $\Delta T = 12 - 10.4 = 1.6\;^{\text{o}}\text{C}$ which is the same as $1.6 \;\text{K}$ .

Heat capacity measures the energy required to raise the temperature of a unit mass of a substance by a unit degree. Therefore

$c = Q / (m \cdot \Delta T) = 56/(11 \times (12 - 10.4)) = 3.2 \; \text{J} \cdot \text{kg}^{-1} \cdot \text{K}^{-1}$

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4 years ago

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