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
alisha [4.7K]
3 years ago
7

A sample of helium gas at a pressure of 0.538 atm and a temperature of 256 °C, occupies a volume of 437 mL. If the gas is cooled

at constant pressure until its volume is 316 mL, the temperature of the gas sample will be
Chemistry
1 answer:
Murrr4er [49]3 years ago
6 0

Answer:

110 °C

Explanation:

The following data were obtained from the question:

Initial pressure (P1) = 0.538 atm

Initial temperature (T1) = 256 °C

Initial volume (V1) = 437 mL.

Final pressure (P2) = constant = 0.538 atm

Final volume (V2) = 316 mL

Final temperature (T2) =?

Next we shall convert 256 °C to Kelvin temperature. This Can be obtained as follow:

T(K) = T(°C) + 273

Initial temperature (T1) = 256 °C

Initial temperature (T1) = 256 °C + 273 = 529 K

Next, we shall determine the new temperature of the gas as illustrated below:

Pressure = constant

Initial temperature (T1) = 529 K

Initial volume (V1) = 437 mL.

Final volume (V2) = 316 mL

Final temperature (T2) =?

Applying the Charles' law equation, we have:

V1 /T1 = V2 /T2

437/529 = 316/T2

Cross multiply

437 × T2 = 529 × 316

437 × T2 = 167164

Divide both side by 437

T2 = 167164 / 437

T2 = 382.5 ≈ 383 K

Finally, we shall convert 383 K to celsius temperature. This can be obtained as follow:

T(°C) = T(K) – 273

T(K) = 383 K

T(°C) = 383 – 273

T(°C) = 110 °C

Therefore, the new temperature of the gas is 110 °C

You might be interested in
An automobile tire at 30°C has a pressure of 3.00 atm. Temperature decreases to -5°C. Assume that there is no volume change in t
dmitriy555 [2]

Answer:

P₂ = 2.7 atm

Explanation:

Given data:

Initial temperature = 30°C

Initial pressure = 3.00 atm

Final temperature = -5°C

Final pressure = ?

Solution:

Initial temperature = 30°C = 30 + 273 = 303 K

Final temperature = -5°C = -5 + 273 = 268 K

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:

3.0 atm / 303 K = P₂/268 K

P₂ = 3.0 atm × 268 K / 303 K

P₂ = 804 atm. K /293 K

P₂ = 2.7 atm

7 0
3 years ago
Calculate the hight of a column of liquid glycerol in meters required to exert the same pressure as 3.02 m if CCl4?
katovenus [111]

Answer:

Approximately 3.81\; \rm m.

Explanation:

Look up the density \rho of carbon tetrachloride, \rm CCl_4, and glycerol:

  • Density of carbon tetrachloride: approximately 1.59\times 10^{3}\; \rm kg \cdot m^{-3}.
  • Density of glycerol: approximately 1.26\times 10^{3}\; \rm kg \cdot m^{-3}.

Let g denote the gravitational field strength. (Typically g \approx 9.81\; \rm N \cdot kg^{-1} near the surface of the earth.) For a column of liquid with a height of h, if the density of the liquid is \rho, the pressure at the bottom of the column would be:

P = \rho\cdot g \cdot h.

The pressure at the bottom of this carbon tetrachloride column would be:

\begin{aligned} P &= \rho \cdot g \cdot h \\ & \approx 1.59\times 10^{3} \; \rm kg \cdot m^{-3} \times 9.81\; \rm N \cdot kg^{-1} \times 3.02 \; \rm m \approx 4.71 \times 10^{4} \; \rm N \cdot m^{-2} \end{aligned}.

Rearrange the equation P = \rho\cdot g \cdot h for h:

\displaystyle h = \frac{P}{\rho \cdot g}.

Apply this equation to calculate the height of the liquid glycerol column:

\begin{aligned}h &= \frac{P}{\rho \cdot g} \\ &\approx \frac{4.71 \times 10^{4}\; \rm N \cdot m^{-2}}{1.26 \times 10^{3}\; \rm kg \cdot m^{-3} \times 9.81\; \rm N \cdot kg^{-1}} \approx 3.81\; \rm m\end{aligned}.

4 0
2 years ago
Isssssssssssssssssssssssssssssss im fat
ale4655 [162]

Answer:

just lose it then lol

Explanation:

6 0
2 years ago
Can someone help me with this?
Rudik [331]
Yeah so you have to start of with converting your first two values into moles (forget the third one)

97.5 g NO * 1 mol/30.01 g NO = 3.25 moles NO

88.0 g O2 * 1 mol/16.00 g O2 = 5.5 moles O2

now we can find the limiting reactant by checking for the amount of product each reactant should give us by using molar ratios

3.25 mol NO * 2 mol NO2/2 mol NO = 3.25 mol NO2

5.5 mol O2 * 2 mol NO2/ 1 mol O2 = 11

so NO is the limiting reactant since it produces less product/gets used up quicker

3.25 mol NO * 2 mol NO2/2molNO = 3.25 mol NO2

so this is our theoretical yield and the question provides us with the actual yield (2.68 moles). since the actual yield is given in moles, we don't have to convert to grams. our percent yield formula goes like: actual yield/theoretical yield * 100

2.68 mol/3.25 mol * 100 = 82.46%
4 0
2 years ago
a compound is composed of only c h and O. Combustion of a 519 gram sample of the compound yields 1.24 grams of CO2 and?
densk [106]

Answer:

C3H3O

Explanation:

Question incomplete needs to be rewritten:

A compound is composed of only C, H, and O. The combustion of a .519-g sample of the compound yields 1.24g of CO_2 and 0.255 g of H_2 O. What is the empirical formula of the compound

We can get the answer through calculations as follows.

From the mass of carbon iv oxide produced, we can get the number of moles of carbon produced. We first divide the mass by the molar mass of carbon iv oxide. The molar mass of carbon iv oxide is 44g/mol

The number of moles of carbon iv oxide is 1.24/44= 0.0282

Since there is only one carbon atom in CO2, the number of moles of carbon is same as above

The mass of carbon in the compound is simply the number of moles multiplied by the atomic mass unit. The atomic mass unit of carbon is 12. The mass of carbon in the compound is thus 12 * 0.0282= 0.338

From the number of moles of water, we can get the number of moles of hydrogen. To get the number of moles of water, we need to divide the mass of water by its molar mass. Its molar mass is 18g/mol. The number of moles here is thus 0.255/18= 0.0142 moles

But there are 2 atoms of hydrogen in 1 mole of water and thus, the number of moles of hydrogen is 2 * 0.0142= 0.0283

The mass of hydrogen is thus 0.0283 * 1 = 0.0283g

The mass of oxygen equals the mass of the compound minus that of hydrogen and that of carbon.

= 0.519 - 0.338 - 0.0283= 0.1527g

The number of moles of oxygen is the mass of oxygen divided by its atomic mass unit.

That equals 0.1527/16= 0.00954375 moles

The empirical formula can be obtained by dividing the number of moles of each by the smallest which is that oxygen 0.00954375 moles

H = 0.0284/0.00954375 = 2.97 = 3

O = 0.00954375/0.00954375= 1

C = 0.0282/0.00954375 = 2.95 = 3

The empirical formula is thus C3H3O

7 0
3 years ago
Other questions:
  • Which of the following would be a warning sign that information about a weight loss medication is not reliable science?
    8·2 answers
  • Why do scientist record observations during an experiment?
    14·1 answer
  • How do you use pedigrees to determine and explain the inheritance of traits?
    6·1 answer
  • What makes urea and breaks down old red blood cells?<br>​
    7·2 answers
  • Pls help Would be much appreciated:)
    15·1 answer
  • When Acid Rain falls on limestone, the rock is eroded and carbon dioxide is produced.
    7·1 answer
  • Which section of the reaction represents the reactants
    14·1 answer
  • Compare the solubility of silver chromate in each of the following aqueous solutions: Clear All 0.10 M AgCH3COO 0.10 M Na2CrO4 0
    10·1 answer
  • What super power would you want to have and why?<br><br> I will give Brainly to the best answer
    7·1 answer
  • What is photolytic decomposition reaction ???​
    9·2 answers
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!