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3 years ago

Help! please! hurry! I will mark brainliest if you get it correct!! NO SPAM!!!!!!

Chemistry

2 answers:

omeli [17]3 years ago

7 0

Answer:

The wavelength λ is the distance between successive peaks in a wave. The frequency f of a wave is the number of complete waves that pass a point in a given time. where c is the speed of light. In your case, λ = 522 nm = 522 × 10⁻⁹ m and c = 2.998 × 10⁸ m·s⁻¹

Explanation:

Troyanec [42]3 years ago

4 0

Answer: 5.747 * 10^14 Hz

Explanation:

Convert 522nm to m = 522 * 10^-9 m (since 1nm=10^-9m)

If c = wavelength * frequency, where c is the speed of light (3.0 * 10^8 m/s), then you can manipulate the equation to solve for frequency (f).

f = c / wavelength

Plug in the given numbers:

f = (3.0 * 10^8) / (10^-9)

f = 5.747 * 10^14 Hz

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1.00 g of a compound is combusted in oxygen and found to give 3.14g of CO2 and 1.29 g of H2O. From these data we can tell thatA.

lora16 [44]

Answer:

the compound contains C, H, and some other element of unknownidentity, so we can’t calculate the empirical formula

Explanation:

Mass of CO2 obtained = 3.14 g

Hence number of moles of CO2 = 3.14g/44.0 g = 0.0714 mol

The mass of the carbon in the sample = 0.0714 mol × 12.0g/mol = 0.857 g

Mass of H2O obtained = 1.29 g

Hence number of moles of H2O = 1.29g/18.0 g = 0.0717 mol

The mass of the carbon in the sample = 0.0717 mol × 1g/mol = 0.0717 g

% by mass of carbon = 0.857/1 ×100 = 85.7 %

% by mass of hydrogen = 0.0717/1 × 100 = 7.17%

Mass of carbon and hydrogen = 85.7 + 7.17 = 92.87 %

Hence, there must be an unidentified element that accounts for (100 - 92.87) = 7.13% of the compound.

5 0

3 years ago

Be sure to answer all parts.

Natali5045456 [20]

Answer:

38.7%

41.3%

20%

Explanation:

The percentage composition helps to know the what percent of the total mass of a compound is made up of each of the constituent elements or groups.

To solve this problem:

find the formula mass by adding the atomic masses of the atoms that makes up the compound.
place the mass contribution of the element or group to the formula mas and multiply by 100;

Compound:

Ca₃(PO₄)₂

Formula mass = 3(40) + 2[31 + 4(16)]

= 120 + 2(95)

= 120 + 190

= 310

%C = $\frac{3(40)}{310}$ x 100 = 38.7%

%P = $\frac{8(16)}{310}$ x 100 = 41.3%

%O = $\frac{2(31)}{310}$ x 200 = 20%

8 0

3 years ago

How much 10% solution and how much 45% solution should be mixed together to make 100 gallons of 25% solution?

Gnoma [55]

x + y = 100

0.10x + 0.45 y =25

eliminate

x + y = 100
x + 4.5 y = 250

-3.5 y = -150
y = 42.85
x = 57.15

hope this helps

5 0

3 years ago

Read 2 more answers

At 570. mmHg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a

marusya05 [52]

Answer:

1560 mmHg is the final pressure

Explanation:

To solve this problem we need to apply the Ideal Gases Law Equation:

P . V = n . R . T

First of all, we need to convert the volume to L, T° to Absolute T° (T°C + 273) and pressure from mmHg to atm

570 mmHg . 1atm/760 mmHg = 0.75 atm

25°C + 273 = 298K

175°C + 273 = 448K

2270 mL . 1L/1000mL = 2.27L

1250 mL . 1L/1000mL = 1.25L

P.V = n . R. T is the main equation but in both cases n and R are constant. We can ignore them, so we make this formula for each situation:

P . V / T = n . R → P₁ . V₁ / T₁ = P₂ . V₂ / T₂

We replace data: 0.75 atm . 2.27L / 298K = P₂ . 1.25L / 448K

(0.75 atm . 2.27L / 298K). 448K = P₂ . 1.25L

2.56 atm.L = P₂ . 1.25L → P₂ = 2.56atm.L / 1.25L = 2.05 atm

We finally convert the atm to mmHg to reach the answer

2.05 atm . 760 mmHg / 1atm = 1556 mmHg ≅ 1560 mmHg

3 0

3 years ago

Can you help me on #14 - #16?

gtnhenbr [62]

15 is b 16 is b and im working on 14

6 0

3 years ago