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2 years ago

PLEASE HELP

Chemistry

2 answers:

Marysya12 [62]2 years ago

6 0

Answer:

Military

Explanation:

I may be wrong but military seems most likely

Maru [420]2 years ago

5 0

Answer: c or 3, "To react to Noriega's attacks".

Explanation: I got right in assignment 2021

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Gas law problem: A gas has a volume of 800 mL at -25℃ and 600 kPa. What would the volume of the gas be at 227℃ and 1000 kPa?

Sati [7]

<h3><u>Answer;</u></h3>

= 930.23 mL

<h3><u>Explanation</u>;</h3>

Using the combined gas law;

P1V1/T1 = P2V2/T2

Where; P1 = 600 kPa, V1 = 800 mL, and T1 = -25 +273 = 258 K, and

V2= ?, P2 = 1000 kPa, and T2 = 227 +273 = 500 K

Thus;

V2 = P1V1T2/T1P2

= (600 ×800 ×500) / (258 × 1000)

= 930.23 mL

5 0

3 years ago

Help. chemistry...........

nasty-shy [4]

<span>The </span>equilibrium<span> will </span>shift<span> to favor the side of the reaction that involves fewer moles of gas.
Its C

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8 0

3 years ago

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An ion from a given element has 24 protons and 22 electrons

musickatia [10]

Hi,

An ion with unequal number of protons and electrons haves a name. A name depends on whether there are more protons than electrons (CATION) or if there are more electrons than protons (ANION).

Hope this helps.
r3t40

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3 years ago

A hydrogen atom has a diameter of about 10 nm. Express this diameter in micrometers, meters, and millimeters.

MariettaO [177]

1) 1 nm = 0.001 µm; one nanometer is equal to 0.001 (10⁻³) micrometer.

d(H) = 10 nm; diameter of hydrogen atom.

d(H) = 10 nm · 0.001 µm/nm.

d(H) = 0.01 µm = 10⁻² µm.

2) 1 nm = 10⁻⁹ m ; one meter is equal to 0.0000000001 (10⁻⁹) meter.

d(H) = 10 nm.

d(H) = 10 nm · 10⁻⁹ m/nm.

d(H) = 0.00000001 m = 10⁻⁸ m.

3) 1 nm = 10⁻⁶ mm ; one nanometer is equal to 0.000001 (10⁻⁶) millimeter.

d(H) = 10 nm · 10⁻⁶ mm/nm.

d(H) = 0.00001 mm = 10⁻⁵ mm.

4 0

3 years ago

Read 2 more answers

A 21.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature ris

Blababa [14]

<u>Answer:</u> The heat capacity of calorimeter is $15.66J/^oC$

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of ethanol = 21.8 g

Molar mass of ethanol = 46.07 g/mol

Putting values in above equation, we get:

$\text{Moles of ethanol}=\frac{21.8g}{46.07g/mol}=0.473mol$

To calculate the enthalpy change of the reaction, we use the equation:

$\Delta H_{rxn}=\frac{q}{n}$

where,

$q$ = amount of heat released = ?

n = number of moles = 0.473 moles

$\Delta H_{rxn}$ = enthalpy change of the reaction = -1235 kJ/mol = $-1235\times 10^3J/mol$ (Conversion factor: 1 kJ = 1000 J)

Putting values in above equation, we get:

$-1235\times 10^3J/mol=\frac{q}{0.473mol}\\\\q=(-1235\times 10^3J/mol\times 0.473mol)=-584.16\times 10^3J$

To calculate the heat capacity of calorimeter, we use the equation:

$q=c\Delta T$

where,

q = heat absorbed by the calorimeter = $584.16\times 10^3J$

c = heat capacity = ?

$\Delta T$ = change in temperature = $T_2-T_1=62.3^oC-25^oC=37.3^oC$

Putting values in above equation, we get:

$584.16\times 10^3J=c\times 37.3^oC\\\\c=\frac{584.16\times 10^3J}{37.3^oC}=15.66J/^oC$

Hence, the heat capacity of calorimeter is $15.66J/^oC$

4 0

3 years ago