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frez [133]
3 years ago
14

The volume of a gas is 22.4 L when the pressure of the atmosphere is 1.00 atm. If the pressure is increased to 1.05 atm, without

changing the temperature, what is the new volume?
K = °C + 273
Question 13 options:

a)

22.4 L


b)

23.5 L


c)

25.2 L


d)

26.3 L
Chemistry
1 answer:
andreyandreev [35.5K]3 years ago
4 0

Answer:

b I think

explanation

they're all false tho

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What state are each of these chemicals in iron steam diamond mercury?
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Fe-- solid

steam -gas

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Stellar fusion produces atoms up to and including ___________ Question 51 options: Helium (atomic number 2) Carbon (atomic numbe
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<h2>Iron (Z = 26)</h2>

Explanation:

  • Stellar fusion is the nuclear reaction that occurs in stars.
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3 years ago
Place the elements below in order of decreasing ionization energy. Aluminum(Al) Chlorine(Cl) Magnesium (Mg) Sulfur(S)
arlik [135]
Chlorine
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7 0
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What criteria are used to classify matter?
Naily [24]
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3 years ago
The following physical constants are for water, H2O.
Delicious77 [7]

Answer:

Q\approx6.4~kJ

Explanation:

Quantity of heat required by 10 gram of ice initially warm it from -5°C to 0°C:

Q_1=m.C_s.\Delta T

here;

mass, m = 10 g

specific heat capacity of ice, C_s=2.09~J.g^{-1}.^{\circ}C^{-1}

change in temperature, \Delta T=(5-0)=5^{o}C

Q_1=10\times2.09\times 5

Q_1=104.5~J

Amount of heat required to melt the ice at 0°C:

Q_2=m.\Delta H_{fus}

where, \Delta H_{fus}=6020~J/mol

we know that no. of moles is = (wt. in gram) \div (molecular mass)

Q_2=\frac{10}{18} \times 6020

Q_2=3344.44~J

Now, the heat required to bring the water to 70°C from 0°C:

Q_3=m.C_L.\Delta T

specific heat of water, C_L=4.18~J/g/^oC

change in temperature, \Delta T=(70-0)=70^oC

Q_3=10\times 4.18\times 70

Q_3=2926~J

Therefore the total heat required to warm 10.0 grams of ice at -5.0°C to a temperature of 70.0°C:

Q=Q_1+Q_2+Q_3

Q=104.5+3344.44+2926

Q=6374.94~J

Q\approx6.4~kJ

8 0
3 years ago
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