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Alex787 [66]
2 years ago
8

PLEASE HELP QUICK!

Chemistry
1 answer:
zvonat [6]2 years ago
6 0

Answer:

1) Mass = 18.864 g

2) V =  2.47 L

Explanation:

1) Given data:

Mass of water produced = ?

Mass of SnO₂ react = 79.0 g

Solution:

SnO₂ + 2H₂   →      Sn + 2H₂O

Number of moles of SnO₂:

Number of moles = mass/molar mass

Number of moles = 79.0 g/ 150.71 g/mol

Number of moles = 0.524mol

Now we will compare the moles of SnO₂ and H₂O

                 SnO₂         :        H₂O

                    1             :          2

                  0.524      :         2/1×0.524 =1.048 mol

Mass of water:

Mass = number of moles × molar mass

Mass = 1.048 mol × 18 g/mol

Mass = 18.864 g

2) Given data:

Volume of oxygen required = ?

Volume of C₃H₈ combust at STP = 0.499 L

Solution:

Chemical equation:

C₃H₈ + 5O₂     →      3CO₂ + 4H₂O

Number of moles of C₃H₈:

PV = nRT

R = general gas constant = 0.0821 atm.L /mol.K

1 atm × 0.499 L = n × 0.0821 atm.L /mol.K × 273.15 K

0.499 L atm.L = n × 22.43 atm.L /mol

n = 0.499 L atm.L / 22.43 atm.L /mol

n = 0.022 mol

Now we will compare the moles of propane and oxygen.

                  C₃H₈        :           O₂

                       1          :           5

                    0.022    :          5/1×0.022 = 0.11 mol

Volume of oxygen required:

PV = nRT

R = general gas constant = 0.0821 atm.L /mol.K

1 atm ×  V = 0.11 mol × 0.0821 atm.L /mol.K × 273.15 K

1 atm ×  V  = 2.47 atm.L

V = 2.47 atm.L  / 1 atm

V =  2.47 L

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Explanation:

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To solve this problem we need to determine the moles of acid that will react, and, using the chemical equation we can determine the moles of NaOH and the volume that a 0.2389M NaOH solution would require to neutralize it.

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Hello!

1.00 L of a gas at STP is compressed to 473 mL. What is the new pressure of gas?

  • <u><em>We have the following data:</em></u>

Vo (initial volume) = 1.00 L  

V (final volume) = 473 mL → 0.473 L  

Po (initial pressure) = 1 atm (pressure exerted by the atmosphere - in STP)  

P (final pressure) = ? (in atm)

  • <u><em>We have an isothermal transformation, that is, its temperature remains constant, if the volume of the gas in the container decreases, so its pressure increases. Applying the data to the equation Boyle-Mariotte, we have:</em></u>

P_0*V_0 = P*V

1*1 = P*0.473

1 = 0.473\:P

0.473\:P = 1

P = \dfrac{1}{0.473}

\boxed{\boxed{P \approx 2.11\:atm}}\:\:\:\:\:\:\bf\green{\checkmark}

<u><em>Answer:  </em></u>

<u><em>The new pressure of the gas is 2.11 atm  </em></u>

___________________________________

\bf\blue{I\:Hope\:this\:helps,\:greetings ...\:Dexteright02!}\:\:\ddot{\smile}

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