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3 years ago

9

3. If all the waves were measured for a period of 5 seconds, which wave had the highest frequency?

1 answer:

Vanyuwa [196]3 years ago

8 0

Answer:

Correct answer is A.

Explanation:

Frequency is the number of oscillations that a wave have per unit time. Since time is measured in seconds, the wave with the highest frequency must register the highest number of oscillation per second. Hence, correct answer is A.

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The bottom number on each element on the Periodic Table is called

Flura [38]

Answer:

The bottom number on each element of the periodic table are called the 4f series or lanthanoids and 5f or actanoids. They are also called inner transition elements.

7 0

3 years ago

Consider the reaction.

Alekssandra [29.7K]

Answer:The correct answer is option C.

Explanation:

$N_2(g)+3H_2(g)\rightarrow 2NH_3(g)$

At STP, 1 mol of gas occupies 22.4 L of volume

So, 100.0 L volume of $NH_3$ will be occupied by :

$\frac{1}{22.4 L}\times 100.0 L=4.4642 moles$

According to reaction 2 moles $NH_3$ are obtained from 1 mole of $N_2$ .

Then,4.4642 moles of $NH_3$ will be obtained from :

$\frac{1}{2}\times 4.4642$ that is 2.2321 moles of $N_2$

Mass of $N_2$ gas:

Moles of $N_2$ gas Molar mass of $N_2$ gas:

$2.2321 mol\times 28 g/mol=62.4988\approx 62.50 g$

Hence, the correct answer is option C.

4 0

3 years ago

Read 2 more answers

The compound consists of 40% carbon and 6.71% hydrogen. Its mass of 1 liter of steam is 2.4 g. What is the formula of the compou

AveGali [126]

I think it is CH2O.

If i'm wrong srry

7 0

3 years ago

Equation for questions 1-4:

Karolina [17]

Answer:

5.625 moles of oxygen, O₂.

Explanation:

The balanced equation for the reaction is given below:

4Al + 3O₂ —> 2Al₂O₃

From the balanced equation above,

4 moles of Al reacted with 3 moles of O₂.

Finally, we shall determine the number of mole of O₂ required to react with 7.5 moles of aluminum, Al. This can be obtained as illustrated below:

From the balanced equation above,

4 moles of Al reacted with 3 moles of O₂.

Therefore, 7.5 moles of Al will react with = (7.5 × 3)/4 = 5.625 moles of O₂.

Thus, 5.625 moles of O₂ is needed for the reaction.

3 0

3 years ago

An experiment shows that a 236 mL gas sample has a mass of 0.443 g at a pressure of 740 mmHg and a temperature of 22 ∘C. What is

aleksley [76]

Answer:

49.2 g/mol

Explanation:

Let's first take account of what we have and convert them into the correct units.

Volume= 236 mL x ( $\frac{1 L}{1000 mL}$ ) = .236 L

Pressure= 740 mm Hg x ( $\frac{1 atm}{760 mm Hg}$ )= 0.97 atm

Temperature= 22C + 273= 295 K

mass= 0.443 g

Molar mass is in grams per mole, or MM= $\frac{mass}{moles}$ or MM= $\frac{m}{n}$ . They're all the same.

We have mass (0.443 g) we just need moles. We can find moles with the ideal gas constant PV=nRT. We want to solve for n, so we'll rearrange it to be

n= $\frac{PV}{RT}$ , where R (constant)= 0.082 L atm mol-1 K-1

Let's plug in what we know.

n= $\frac{(0.97 atm)(0.236 L)}{(0.082)(295K)}$

n= 0.009 mol

Let's look back at MM= $\frac{m}{n}$ and plug in what we know.

MM= $\frac{0.443 g}{0.009 mol}$

MM= 49.2 g/mol

3 0

3 years ago