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mars1129 [50]
3 years ago
15

What is true of a sample of gas as temperature is increased?

Chemistry
2 answers:
aniked [119]3 years ago
6 0

Answer:

The particles move faster, and their average kinetic energy increases.

Explanation:

When the temperature of gases increases the reaction rates will increase. Molecules of gases will be furnished with higher kinetic energy. Kinetic energy is directly proportional to temperature. Increase in temperature causes the frequency of ordinary collisions and effective collisions per unit time to increase. This leads to a surge in kinetic energy too.

Paul [167]3 years ago
6 0

Answer: The particles move faster, and their average kinetic energy increases.

Explanation:

Kinetic energy is the energy possessed by an object by virtue of its motion.

Average kinetic energy is defined as the average of the kinetic energies of all the particles present in a system. It is determined by the equation:

K=\frac{3RT}{2}

K= kinetic energy

R= gas constant

T= temperature  

From above, it is visible that kinetic energy is directly related to the temperature of the system.

So, if temperature is more, average kinetic energy of the system is more and thus speed of the molecules will be more.Thus the molecules will move faster.

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A student determines that she used 0.0665 mol of sodium hydroxide (NaOH) to completely titrate 25.00 mL of sulfuric acid solutio
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To determine the concentration of one solution which is specifically basic or acidic solution through taking advantage on its points of equivalence, titration analysis is done.

Let us determine the reaction for the titration below:

2NaOH +2H2SO4 = Na2SO4 +2H2O

 

So,

0.0665 mol NaOH (2 mol H2SO4/ 2mol NaOH) / .025 L solution 

= 2.62 M H2SO4


The answer is the fourth option: 

<span>2.62 M</span>
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3 years ago
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A trial of this decomposition experiment, using different quantities of reactants than those listed in the question above produc
Paul [167]

Answer : The volume of O_2(g) produced at standard conditions of temperature and pressure is 0.2422 L

Explanation :

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}

where,

P_1 = initial pressure of O_2 gas = (740-22.4) torr = 717.6 torr

P_2 = final pressure of O_2 gas at STP= 760 torr

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V_2 = final volume of O_2 gas at STP = ?

T_1 = initial temperature of O_2 gas = 25^oC=273+25=298K

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Now put all the given values in the above equation, we get:

\frac{717.6torr\times 280mL}{298K}=\frac{760torr\times V_2}{273K}

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5 0
3 years ago
What is the net ionic equation for 2AgNO3 + 2NaOH = Ag2O + 2NaNO3 + H2O
soldi70 [24.7K]

Answer:

2Ag⁺ (aq) + 2OH⁻ (aq) → Ag₂O (s) + H₂O (l)

Explanation:

Step 1: RxN

2AgNO₃ + 2NaOH → Ag₂O + 2NaNO₃ + H₂O

Step 2: Define states of matter

2AgNO₃ (aq) + 2NaOH (aq) → Ag₂O (s) + 2NaNO₃ (aq) + H₂O (l)

Step 3: Total Ionic Equation

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7 0
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Calculate the moles and grams of solute in each solution. D. 2.0 L of 0.30M Na2SO4. I already have A, B, and C. Thanks!
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C(Concentration) = 0.30 moles / L
V ( Volume) = 2 L
n = ??
n = C * V
n = 0.30 mol / L * 2 L
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1S   = 32 * 1 = 32 grams
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given mass = molar mass * mols
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85.2 are in a 2 L solution that has a concentration of 0.6 mol/L


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