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Rom4ik [11]
2 years ago
7

The volume of a sample of oxygen is 300.0 mL, when the pressure is 1.00 atm and the temperature is 300K. At what pressure will t

he volume be 1000.0 mL and a temperature of 500K?
Chemistry
1 answer:
Brut [27]2 years ago
4 0

Answer:

The new pressure is 0.5 atm

Explanation:

Step 1: Data given

Volume of oxygen = 300 mL = 0.300 L

Pressure = 1.00 atm

Temperature = 300 K

The volume increases to 1000mL = 1.00 L

The temperature increases to 500 K

Step 2: Calculate the new pressure

(P1*V1)/T1 = (P2*V2)/T2

⇒with P1 = the initial pressure = 1.00 atm

⇒with V1 = the initial volume = 0.300 L

⇒with T1 = the initial temperature = 300 K

⇒with P2 = the new pressure = TO BE DETERMINED

⇒with V2 = the increased volume = 1.00 L

⇒with T2 = the increased temperature = 500 K

(1.00 atm* 0.300 L)/300 K = (P2 * 1.00L) / 500 K

P2 = (1.00 *0.300 * 500) / (300 *1.00)

P2 = 0.5 atm

The new pressure is 0.5 atm

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According to the following reaction, how many grams of nitrogen monoxide will be formed upon the complete reaction of 31.0 grams
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Explanation:

The balanced chemical equation is:

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Number of moles will be calculated.

31 grams of oxygen is given

atomic weight of oxygen gas i.e O2 = 32gm/mole

The molar mass of oxygen gas is 32 grams/mole which is equal to one mole of the molecule.

Number of moles (n) = \frac{mass}{atomic mass of one mole of the substance}

                             n=    \frac{31}{32}

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5 moles of oxygen yielded 4 moles of NO

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x = 0.774 moles of NO will be formed.

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