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timurjin [86]
3 years ago
5

Question 6 of 10

Chemistry
1 answer:
lesya [120]3 years ago
7 0
The answer is B. Molecules move more quickly as temperature increases.

When Allmond molecular motion stops, that is considered absolute zero. That does not mean that it cannot get colder, disapproving A.

C is just wrong.

D says when molecular motion stops the temperature STARTS to decrease, it was decreasing before it got there.
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5 0
3 years ago
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a mixture of gases contains He (g) and Ne (g). the total pressure of the atmosphere in the container is 600 mmHg and the partial
aliina [53]

Answer:

161 mmHg

Explanation:

Ptotal= PHe +PNe

PHe= Ptotal-PNe

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PHe=161 mmHg

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3 years ago
7. A cyclist starting from rest accelerates at a rate of 6 m/s until she reaches 30 m/s. How long
Hunter-Best [27]

Answer:

Explanation:

The given values are:

a= 6m/s²

u= 0 m/s

v = 30 m/s

t= ?

The formula is :

a=\frac{v-u}{t}

thus,

t=\frac{v-u}{a}\\t=\frac{30-0}{6}\\t= 5 seconds

4 0
3 years ago
A change that produces one or more new substances is called _____.
Vesnalui [34]

Answer:

the answer is c

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a chemical change mean it changes it for ever and a physical change mean it can be changed back and evaporation means it turns solid water in to gas hope this helps

7 0
3 years ago
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Nicotine, a component of tobacco, is composed of c, h, and n. A 2.625-mg sample of nicotine was combusted, producing 7.1210 mg o
Vikki [24]

The mass sample of nicotine combusted = 2.625 mg  (given)

Mass of CO_2 produced = 7.1210 mg  (given)

Mass of H_2O produced = 2.042 mg  (given)

Molar mass of CO_2 = 44 g/mol

Molar mass of H_2O = 18 g/mol

Percentage of Carbon = \frac{12 g}{44 g/mol}\times \frac{7.120 mg of CO_2}{2.625 mg sample}\times 100 = 74.04%

Percentage of hydrogen = \frac{2 g}{18 g/mol}\times \frac{2.04 mg of H_2O}{2.625 mg sample}\times 100 = 8.62%

Now, for percentage of nitrogen = 100 - (74.04+8.62) = 17.34%

Calculating the moles of each element:

Number of moles = \frac{given mass}{Molar mass}

  • For C

\frac{74.04 g}{12 g/mol} = 6.17 mol

  • For H

\frac{8.62 g}{1 g/mol} = 8.62 mol

  • For N

\frac{17.34 g}{14 g/mol} = 1.24 mol

Dividing with the smallest mole value to calculate the molar ratio of each element:

C_{\frac{6.17}{1.24}} = C_{4.9} = C_5

H_{\frac{8.62}{1.24}} = H_{6.9} = H_7

N_{\frac{1.24}{1.24}} = N_1

Hence, the empirical formula for nicotine is C_5H_7N.

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3 years ago
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