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2 years ago

I AMMMM GIVING 45 POINTSSSS PLSSS HELPPPPPPPP

Chemistry

1 answer:

Westkost [7]2 years ago

8 0

Answer:

mNaNO3 =765g

Explanation:

First, we write the balanced chemical equation representing the chemical reaction that happened between aluminum nitrate and sodium chloride.

Balanced chemical equation:

AL(NO3)3+3NaCl ⟶ 3 NaNO3+AlCl3

According to the equation, each mole of aluminum nitrate requires three moles of sodium chloride. Thus, the required number of moles of sodium chloride is

4 Mol ⋅ 3 = 12mol

Based on the data provided in the table, there were 9 moles of sodium chloride used in the reaction, which was not enough for the entirety of aluminum nitrate to react. So, sodium chloride must have been the limiting reactant.

Therefore, we use the number of moles (n) of sodium chloride to calculate the number of moles of sodium nitrate, which has a 1:1 ratio with sodium chloride.

Number of moles sodium nitrate:

nNaNO3=nNaCl

nNaNO3 = 9 mol

We can also calculate the mass (m) of sodium nitrate that was produced by multiplying its number of moles by its molar mass (MM), 85.00g/mol.

Mass of sodium nitrate produced:

mNaNO3 = nNaNO3 ⋅ MMNaNO3

mNaNO3 = 9 mol ⋅ 85.00 g/mol

mNaNO3 =765g

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The ionization energy

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A sample in the laboratory is found to contain 3.36 grams of hydrogen, 20.00 grams of carbon, and 26.64 grams of oxygen. The mol

KonstantinChe [14]

Answer:

Empirical formula is CH₂O.

Molecular formula = C₆H₁₂O₆

Explanation:

Given data:

Mass of hydrogen = 3.36 g

Mass of carbon = 20.00 g

Mass of oxygen = 26.64 g

Molar mass of compound = 180.156 g/mol

Empirical formula = ?

Molecular formula = ?

Solution:

Empirical formula:

It is the simplest formula gives the ratio of atoms of different elements in small whole number

Number of gram atoms of H = 3.36 / 1.01 = 3.3

Number of gram atoms of O = 26.64 / 16 = 1.7

Number of gram atoms of C = 20 / 12 = 1.7

Atomic ratio:

C : H : O

1.7/1.7 : 3.3/1.7 : 1.7/1.7

1 : 2 : 1

C : H : O = 1 : 2 : 1

Empirical formula is CH₂O.

Molecular formula:

Molecular formula = n (empirical formula)

n = molar mass of compound / empirical formula mass

Empirical formula mass = CH₂O = 12×1 + 2× + 16

Empirical formula mass = 30

n = 180.156 / 30

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3 years ago

If the detector is capturing 3.3×108 photons per second at this wavelength, what is the total energy of the photons detected in

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Answer:

The total energy of the photons detected in one hour is 7.04*10⁻¹¹ J

Explanation:

The energy carried by electromagnetic radiation is displaced by waves. This energy is not continuous, but is transmitted grouped into small "quanta" of energy called photons. The energy (E) carried by electromagnetic radiation can be measured in Joules (J). Frequency (ν or f) is the number of times a wave oscillates in one second and is measured in cycles / second or hertz (Hz). The frequency is directly proportional to the energy carried by a radiation, according to the equation: E = h.f, (where h is the Planck constant = 6.63 · 10⁻³⁴ J / s).

Wavelength is the minimum distance between two successive points on the wave that are in the same state of vibration. it is expressed in units of length (m). In light and other electromagnetic waves that propagate at the speed of light (c), the frequency would be equal to the speed of light (≈ 3 × 10⁸ m / s) between the wavelength :

$f=\frac{speed of light}{wavelength}$

So:

$E=\frac{h*speed of light}{wavelength}$

In this case, the wavelength is 3.35mm=3.35*10⁻³m and the energy per photon is:

$E=\frac{6.63*10^{-34}*3*10^{8}}{3.35*10^{-3} }$

E=5.93*10⁻²³ $\frac{J}{proton}$

The detector is capturing 3.3*10⁸ photons per second. So, in 1 hour:

$E=5.93*10^{-23} \frac{J}{proton} *3.3*10^{8} \frac{proton}{s} *\frac{60}{1} \frac{s}{minute} *\frac{60}{1} \frac{minute}{hr}$

E=7.04*10⁻¹¹ $\frac{J}{hr}$

The total energy of the photons detected in one hour is 7.04*10⁻¹¹ J

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