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Aleksandr [31]
3 years ago
12

The temperature is -14°C the air pressure in an automobile tire is 149K PA if the volume does not change what is the pressure af

ter the tire is heated to 17.3°C
Chemistry
1 answer:
Jet001 [13]3 years ago
4 0

Answer: The pressure after the tire is heated to 17.3°C is 167 kPa

Explanation:

To calculate the final temperature of the system, we use the equation given by Gay-Lussac Law. This law states that pressure of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

\frac{P_1}{T_1}=\frac{P_2}{T_2}

where,

P_1\text{ and }T_1 are the initial pressure and temperature of the gas.

P_2\text{ and }T_2 are the final pressure and temperature of the gas.

We are given:

P_1=149kPa\\T_1=-14^0C=(273-14)=259K\\P_2=?=27.5psi\\T_2=17.3^0C=(273+17.3)=290.3K

Putting values in above equation, we get:

\frac{149}{259}=\frac{P_2}{290.3}\\\\P_2=167kPa

Hence, the pressure after the tire is heated to 17.3°C is 167 kPa

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Answer:

True

Explanation:

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The distance that the molecules move depends on their solubility in the solvent and the size of the molecules. Heavy molecules will travel slower and therefore travel a shorter distance in the time the chromatography is run.

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3 years ago
An element's atomic number is 87. how many protons would an atom of this element have
andreev551 [17]
atomic number is equal to proton number
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5 0
3 years ago
Answer True or False for each of the following statements. (a) The carburization surface was maintained at slightly less than 0.
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verdadero/a

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verdadero/c

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2 years ago
If 14.5 g of MnO4- (permanganate) react with manganese (II) hydroxide how many grams of manganese (IV) oxide will be produced? T
Veronika [31]

Answer:

m_{MnO_2}=21.2gMnO_2

Explanation:

Hello,

In this case, given the balanced reaction:

2MnO_4^-+2Mn(OH)_2\rightarrow 4MnO_2+2OH^-+H_2O

We can see a 2:4 mole ration between permanganate ion (118.9 g/mol) and manganese (IV) oxide (86.9 g/mol), that is why the resulting mas of this last one turns out:

m_{MnO_2}=14.5gMnO_4^-*\frac{1molMnO_4^-}{118.9gMnO_4^-}*\frac{4MnO_2}{2molMnO_4^-}  *\frac{86.9gMnO_2}{1molMnO_2} \\\\m_{MnO_2}=21.2gMnO_2

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5 0
3 years ago
(a) Write the dissolution reaction for solid Na2CO3 below. (Use the lowest possible coefficients. Include states-of-matter under
Andreas93 [3]

<u>Answer:</u>

<u>For a:</u> The chemical equation for the dissolution of sodium carbonate is Na_2CO_3(s)\rightarrow Na_2CO_3(aq.)

<u>For b:</u> The net acid-base reaction is CO_3^{2-}(aq.)+H_2O(l)\rightarrow OH^-(aq.)+HCO_3^-(aq.)

<u>Explanation:</u>

  • <u>For a:</u>

Dissolution reaction is defined as the reaction in which a solid compound gets dissolved in water to form aqueous solution.

The chemical equation for the dissolution of sodium carbonate follows:

Na_2CO_3(s)\rightarrow Na_2CO_3(aq.)

Ionization reaction is defined as the reaction in which an ionic compound dissociates into its ions when dissolved in aqueous solution.

The chemical equation for the ionization of sodium carbonate follows:

Na_2CO_3(aq.)\rightarrow 2Na^+(aq.)+CO_3^{3-}(aq.)

  • <u>For b:</u>

Now, the anion formed which is CO_3^{2-} reacts with water to form conjugate acid.

The chemical equation for the reaction of anion with water follows:

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Hence, the net acid-base reaction of the anion formed and water is written above.

3 0
3 years ago
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