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Norma-Jean [14]
3 years ago
13

2) what is the mass of 6.02 x 1023 atoms of arsenic?

Chemistry
1 answer:
zzz [600]3 years ago
6 0
Data:
Arsenic Molar Mass = 74,9216 ≈ 75 u (<span>atomic mass unit)</span>

Solving:

1 mole of arsenic → 75g ------------ 6,02*10²³ molecules
..................................X -------------- 1 molecule

6,02*10²³X = 75
x = \frac{75}{6,02*10^{23}}
\boxed{x \approx 1,24*10^{24}grams}
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I believe it's 1. 9.
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What is the temperature of CO2 gas if the average speed (actually the root-mean-square speed) of the molecules is 750 m/s?
erastova [34]

Answer:

992.302 K

Explanation:

V(rms) = 750 m/s

V(rms) = √(3RT / M)

V = velocity of the gas

R = ideal gas constant = 8.314 J/mol.K

T = temperature of the gas

M = molar mass of the gas

Molar mass of CO₂ = [12 + (16*2)] = 12+32 = 44g/mol

Molar mass = 0.044kg/mol

From

½ M*V² = 3 / 2 RT

MV² = 3RT

K = constant

V² = 3RT / M

V = √(3RT / M)

So, from V = √(3RT / M)

V² = 3RT / M

V² * M = 3RT

T = (V² * M) / 3R

T = (750² * 0.044) / 3 * 8.314

T = 24750000 / 24.942

T = 992.302K

The temperature of the gas is 992.302K

Note : molar mass of the gas was converted from g/mol to kg/mol so the value can change depending on whichever one you use.

3 0
3 years ago
Wood with a mass of 3.0 grams was burned in an open dish. The ashes weighed 1.2 grams.
mr_godi [17]

The rest of the wood was burned into gases of equivalent weight.

<u>Explanation</u>:

The rest of the wood was burned into gases of equivalent weight.

  • When wood is burnt in the open air, with the help of oxygen and heat, it is transformed into carbon dioxide, water vapor, and ashes.
  • Ignition and combustion of wood mainly depend on pyrolysis which is also known as thermal combustion.
  • The loss in weight of the ashes is due to the fact that gases and water vapor are also formed due to the combustion of wood.

7 0
3 years ago
How do we detect the change in energy?
IrinaVladis [17]
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MARK ME AS BRAINLIEST
3 0
2 years ago
A compound contains 78.14% B and 21.86% H by mass and has a molar mass of 27.67 g/mol. What is the molecular formula of the comp
ziro4ka [17]

Answer:

The molecular formula of the compound is B₂H₆

Explanation:

From the question given above, the following data were obtained:

Composition of Boron (B) = 78.14%

Composition of Hydrogen (H) = 21.86%

Molar mass of compound = 27.67 g/mol

Molecular formula =?

Next, we shall determine the empirical formula of the compound. This can be obtained as follow:

B = 78.14%

H = 21.86%

Divide by their molar mass

B = 78.14 / 11 = 7.104

H = 21.86 / 1 = 21.86

Divide by the smallest

B = 7.104 / 7.104 = 1

H = 21.86 / 7.104 = 3

Thus, the empirical formula of the compound is BH₃

Finally, we shall determine the molecular formula of the compound. This can be obtained as illustrated below:

Molecular formula = empirical formula × n

Molecular formula = [BH₃]ₙ

Thus, we shall determine the value of n to obtain the molecular formula. The value of n can be obtained as follow:

[BH₃]ₙ = 27.67

[11 + (3×1)]n = 27.67

[11 + 3]n = 27.67

14n = 27.67

Divide both side by 14

n = 27.67 / 14

n = 2

Molecular formula = [BH₃]ₙ

Molecular formula = [BH₃]₂

Molecular formula = B₂H₆

4 0
3 years ago
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