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2 years ago

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Chemistry

1 answer:

ddd [48]2 years ago

7 0

Answer:

116 °C

Explanation:

The given parameters of the Substance Q are;

The boiling point of Q = 445°

The substance Q is a solid at room temperature

Given that Q has a single fixed boiling point, Q, is suspected to be a pure substance, and it will therefore also have a fixed single melting point above room temperature;

Therefore, the best option is option C. 116 °C, which is above a single temperature value above 116 °C

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My swimming pool is rectangular (16 feet by 34 feet) and has a depth of 6 feet. Lets imagine that my pool water is full to the t

Reil [10]

Answer:

Number of moles of photons required = 5.04 × 10⁴ moles

Explanation:

The energy of a photon can be calculated from Planck's equation E = hc/λ

Where h = 6.63 × 10-³⁴ Js and c, the velocity of light = 3.0 × 10⁸ m/s

Energy of one mole of photons = N₀ × hc/λ

wavelength of photon, λ = 520 nm = 5.20 × 10-⁷ m

Energy of one mole of photons = 6.02 × 10²³ × 6.63 × 10−³⁴ × 3 × 10⁸/5.20 × 10-⁷

Energy of one mole of photons = 2.30 × 10⁵ J/mol

Energy required to raise the temperature of a given mass of a substance, E = mcΔT

Where m is mass of substance, c is specific heat capacity, ΔT is temperature difference

Mass ofnwternin the pool = volume × density

Volume of water = Volume of swimming pool

Volume of water = 16 × 34 × 6 ft³ = 3264 ft³

1 ft³ = 28316.8 cm³; 3264 ft³ = 28316.8 × 3264 = 92426035.2 cm³

Density of water = 1 g/cm³

Mass of water = 92426035.2 cm³ × 1 g/cm³ = 92426035.2g

ΔT = 80°C - 50°C = 30°C, c = 4.18 J/g/K

Energy required to raise 92426035.2 g water by 30° C = 92426035.2 × 4.18 × 30

Energy required = 1.16 × 10¹⁰ J

Hence, number of moles of photons required = 1.16 × 10¹⁰ J/2.30 × 10⁵ J/mol

Number of moles of photons required = 5.04 × 10⁴ moles

5 0

3 years ago

While following the Dumas method, a student assumes that the contents of the container are the same temperature as the water bat

Nataliya [291]

Answer:

Explanation:

the Molar mass will be smaller as the content of the container is not directly proportional to the temperature of the water bath.

5 0

3 years ago

Stoichiometric coefficients indicate the ratio between ________of given substances in a chemical reaction

Cloud [144]

Answer:

Explanation:

7 0

3 years ago

What is the molarity of a solution that contains 1000.0 mg of AgNO3 that has been dissolved in 500 mL of water

Vaselesa [24]

0.012moldm⁻³

Explanation:

Given parameters:

Mass of AgNO₃ = 1000mg

Volume of water = 500mL

Unknown:

Molarity of solution = ?

Solution:

The molarity of a solution is the number of moles of a solute dissolved in volume of solvent.

Molarity = $\frac{xnumber of moles}{Volume}$

Number of moles of AgNO₃ = ?

Number of moles = $\frac{mass}{molar mass}$

Molar mass of AgNO₃ = 108 + 14 + 3(16) = 170g/mol

convert mass to g;

1000mg = 1g

Number of moles = $\frac{1}{170}$ = 0.00588moles

convert the given volume to dm³;

1000mL = 1dm³;

500mL = 0.5dm³

Now solve;

Molarity = $\frac{0.00588}{0.5}$ = 0.012moldm⁻³

learn more:

Molarity brainly.com/question/9324116

#learnwithBrainly

4 0

3 years ago

In 1909 Fritz Haber discovered the workable conditions under which nitrogen, N2(g), and hydrogen, H2(g), would combine using to

labwork [276]

Answer : 51.8 g of nitrogen are needed to produce 100 grams of ammonia gas.

Solution : Given,

Mass of $NH_3$ = 100 g

Molar mass of $NH_3$ = 27 g/mole

Molar mass of $N_2$ = 28 g/mole

First we have to calculate moles of $NH_3$ .

$\text{ Moles of }NH_3=\frac{\text{ Mass of }NH_3}{\text{ Molar mass of }NH_3}= \frac{100g}{27g/mole}=3.7moles$

The given balanced chemical reaction is,

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

From the given reaction, we conclude that

2 moles of $NH_3$ produced from 1 mole of $N_2$

3.7 moles of $NH_3$ produced from $\frac{1mole}{2mole}\times 3.7mole=1.85moles$ of $N_2$

Now we have to calculate the mass of $N_2$ .

Mass of $N_2$ = Moles of $N_2$ × Molar mass of $N_2$

Mass of $N_2$ = 1.85 mole × 28 g/mole = 51.8 g

Therefore, 51.8 g of nitrogen are needed to produce 100 grams of ammonia gas.

5 0

2 years ago