1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Eddi Din [679]
3 years ago
12

1. A gas at 24.0 Celsius and.900 atm fills a 0.95 Liter container.

Chemistry
1 answer:
dangina [55]3 years ago
4 0

Answer:

P₂ = 1.05 atm

Explanation:

Given data:

Initial temperature = 24.0 °C (24+273 = 297 K)

Initial pressure = 0.900 atm

Final pressure = ?

Final temperature = 75 °C (75 + 273 =348 K)

Volume = constant

Solution:

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

0.900 atm / 297 K = P₂/348 K

P₂ = 0.900 atm × 348 K / 297 K

P₂ = 313.2 atm. K /297 K

P₂ = 1.05 atm

You might be interested in
A reaction occurs via the following sequence of elementary steps. What is the reaction intermediate?
Trava [24]

Answer:

C is the reaction intermediate.

Explanation:

A reaction intermediate is a molecular structure that is formed during the reaction but then is converted in the final products.

Usually, these reaction intermediates are unestable and, for that reason, the lifetime of these structures is low.

In the reaction, you can see in the first step C is produced, but also, in the second step reacts producing D. As is produced and, immediately consumed,

<h3>C is the reaction intermediate.</h3>
3 0
3 years ago
How many moles of H2O2 are needed to react with 1.07 moles of N2H4?
I am Lyosha [343]

Answer:

2.14 moles of H₂O₂ are required

Explanation:

Given data:

Number of moles of H₂O₂ required = ?

Number of moles of N₂H₄ available = 1.07 mol

Solution:

Chemical equation:

N₂H₄  +   2H₂O₂       →   N₂ +  4H₂O

now we will compare the moles of H₂O₂ and N₂H₄

                          N₂H₄     :      H₂O₂  

                            1           :        2

                            1.07      :         2×1.07 = 2.14 mol

                   

6 0
3 years ago
Calculate in gramm the mass of 0.1 mole of hydrochloric acid(h=1 ,cl=35.5)​
babunello [35]

Answer:

mass of HCl = 3.65 g

Explanation:

Data Given:

Moles of hydrochloric acid HCl = 0.1 mole

Mass in grams of hydrochloric acid HCl = ?

Solution:

Mole Formula

                  no. of moles = Mass in grams / molar mass

To find Mass in grams rearrange the above Formula

                Mass in grams = no. of moles x molar mass . . . . . . . (1)

Molar mass of HCl = 1 + 35.5 = 36.5 g/mol

Put values in equation 1

              Mass in grams = 0.1 mole x 36.5 g/mol

              Mass in grams = 3.65 g

mass of HCl = 3.65 g

6 0
3 years ago
3 , from
Mazyrski [523]

Answer:

troposphere

stratosphere

exosphere

4 0
2 years ago
Read 2 more answers
What type of reaction is Zn + CuCl2 → Cu + ZnCl2?​
Shalnov [3]

Answer:

Its single - displacement.

Explanation:

4 0
3 years ago
Other questions:
  • What is an astronomical unit? Why is this unit used to measure distances in the solar system?
    6·2 answers
  • Empirical formula for C2H6O4
    5·1 answer
  • In a model of an atom, where would I find a valence electron<br><br><br> Help
    9·1 answer
  • Nuclear fusion please help :/
    9·1 answer
  • Pt5 science......<br><br> Select correct answer ♡ !
    12·2 answers
  • Plz help..........................
    12·1 answer
  • Where would you expect to find the 1H NMR signal of (CH3)2Mg relative to the TMS signal? (Hint: Magnesium is less electronegativ
    14·1 answer
  • What does this mean and how do I answer?
    15·1 answer
  • What is the percent of O in<br> CO2?<br> (C = 12.01 amu, O = 16.00 amu)<br> [? ]%
    5·2 answers
  • The multiple covalent bond in a molecule of 1-butene is a.
    9·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!