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3 years ago

6

Ann and Jesse's mom is driving them to school. They are listening to music on an FM radio station. When they ride in the car wit

h their father,
they sometimes listen to AM radio. Ann wants to find out the difference between AM and FM radio signals. She finds a diagram in an online
search

1 answer:

Svet_ta [14]3 years ago

3 0

Answer: it they are both in the same place

Explanation:I don’t know and don’t care loser

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Which of the following would be the most difficult to compress?

Alchen [17]

The hardest to compress here would be the brick

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3 years ago

Read 2 more answers

frozen [14]

Given question is incomplete. The complete question is as follows.

Pentaborane ( $B_{5}H_{9}$ ) is a colorless highly reactive liquid that will burst into flames when exposed to oxygen.the reaction is:

$2B_{5}H_{9}(l) + 12O_{2} \rightarrow 5B_{2}O_{2}(s) + 9H_{2}O(l)$

Calculate the kilojoules of heat released per gram of the compound reacted with oxygen.the standard enthalpy of formation $B_{5}H_{9}(l)$ , $B_{2}O_{3}(s)$ , and $H_{2}O(l)$ are 73.2, -1271.94, and -285.83 kJ/mol, respectively.

Explanation:

As the given reaction is as follows.

$2B_{5}H_{9}(l) + 12O_{2} \rightarrow 5B_{2}O_{2}(s) + 9H_{2}O(l)$

Therefore, formula to calculate the heat energy released is as follows.

$\Delta H = \sum H_{products} - \Delta H_{reactants}$

Hence, putting the given values into the above formula is as follows.

$\Delta H = \sum H_{products} - \Delta H_{reactants}$

= $5 \times (-1271.94 kJ/mol) + 9 \times (-285.83 kJ/mol) - 2 \times (73.2 kJ/mol) - 12(0)$

= -9078.59 kJ/mol

Since, 2 moles of Pentaborane reacts with oxygen. Therefore, heat of reaction for 2 moles of Pentaborane is calculated as follows.

$\frac{\Delta H}{2 \times \text{molar mass of pentaborane}}$

$\frac{-9078.59 kJ/mol}{2 \times 63.12 g/mol}$

= -71.915 kJ/g

Thus, we can conclude that heat released per gram of the compound reacted with oxygen is 71.915 kJ/g.

8 0

3 years ago

How many atoms are in 52.3 g of lithium hypochlorite (LiClO)?

garri49 [273]

Answer:

1.62 × 10²⁴ atoms are in 52.3 g of lithium hypochlorite.

Explanation:

To find the amount of atoms that are in 52.3 g of lithium hypochlorite, we must first find the amount of moles. We do this by dividing by the molar mass of lithium hypochlorite.

52.3 g ÷ 58.4 g/mol = 0.896 mol

Next we must find the amount of formula units, we do this be multiplying by Avagadro's number.

0.896 mol × 6.02 × 10²³ = 5.39 × 10²³ f.u.

Now to get the amount of atoms we can multiply the amount of formula units by the amout of atoms in one formula unit.

5.39 × 10²³ f.u. × 3 atom/f.u. = 1.62 × 10²⁴ atoms

1.62 × 10²⁴ atoms are in 52.3 g of lithium hypochlorite.

7 0

3 years ago

A 100.0g sample of tin is heated to 100.0 oC (Celsius) and is placed in a coffee cup calorimeter containing 150. g of water at 2

Snowcat [4.5K]

Explanation:

It is known that specific heat of water is 4.184 $J/g^{o}C$ and atomic mass of tin is 118.7 g/mol. For the given situation,

$Q_{lost} = Q_{gained}$

Let us assume that,

$m_{1}$ = mass of Sn

$m_{2}$ = mass of $H_{2}O$

Therefore, heat energy expression for heat lost and gained is as follows.

$Q_{lost} = Q_{gained}$

$m_{1}C_{1}(T_{2} - T_{1}) = m_{2}C_{2}(T_{1} - T_{2})$

$100 g \times C_{1} \times (100^{o}C - 27.4^{o}C) = 150 g \times 4.184 /g^{o}C \times (27.4^{o}C - 25^{o}C)$

$7260C_{1} = 150 \times 4.184 \times 2.4$

$C_{1} = \frac{1506.24}{7260}$

= 0.207 $J/g^{o}C$

For, 118.7 g the specific heat of tin will be calculated as follows.

$C_{1} = 0.207 J/g^{o}C \times 118.7 g$

= 24.5 $J/mol^{o}C$

Thus, we can conclude that specific heat of tin is 24.5 $J/mol^{o}C$ .

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3 years ago

Theories change because new technology improves our ability to observe the natural world.

rewona [7]

Answer:

True

Theories change because new technology improves our ability to observe the natural world. answer choices.

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3 years ago