what is the motor system of atm machine?
1. what is the motor system of atm machine?
Explanation:
heeh! yan na mga prii heeh!
2. How does the ATM make the system secure?
Answer:
There are guards on there side is that to make sure safe and sound.
Answer:
its secured by the password
edit:( Atm card or machine?)
3. 1. A balloon has a pressure of 2.05 atm and at 28°C. If the temperature is reduced to 16°C, what will be the new pressure of the balloon? a. 3.97 atm b. 1.97 atm c. 2.97 atm d. 4.97 atm
Answer:
b. 1.97 atm
Explanation:
[tex]\frac{2.05(273+16)}{273+28} = 1.96827 atm = 1.97 atm[/tex]
4. The volume of a gas at 27 °C is 300 mL. If the pressure remains constant, what is the new volume if the temperature is raised to 100 °C? A. 3.0 atm B. 2.5 atm C. 2.0 atm D. 1.5 atm
Answer:
Menurut saya c
Explanation:
Saya tidak pernah melakukannya
5. Three gases, Ar, N2 and H2 are mixed in a 500L container. Ar has a pressure of 2 atm, N2 has a pressure of 3 atm and H2 has pressure of 2 atm. What is the total pressure in the container?a. 2 atm b. 3 atm c. 5 atm d. 7 atm.
Answer:
[tex] \therefore [/tex] The total pressure in the container is 7 atm (D.)
Explanation:
We have three gases which is [tex] \rm{Ar, \ N_2, \ and \ H_2} [/tex] they all mixed in 500L. So, we want to there total pressure. To know how many total of pressure in the container, we will use Dalton's Equation.
[tex] \boxed{\bold{P_{Total} = P_1 + P_2 + P_3...}}[/tex][tex] \begin{gathered}\begin{gathered}\begin{aligned} & \bold{Thus, \ the \ given \ are:} \\ & \quad \boxed{\begin{array}{l} \Longrightarrow \rm{P_1} = 2 \ atm \\ \Longrightarrow \rm{P_2} = 3 \ atm \\ \Longrightarrow \rm{P_3} = 2 \ atm \end{array}}\, \\ \end{aligned} \end{gathered}\end{gathered} [/tex]
Substitute it to the formula
[tex] \rm{P_{Total} = 2 \ atm + 3 \ atm + 2 \ atm} [/tex][tex] \rm{P_{Total} = 4 \ atm + 3 \ atm} [/tex][tex] \rm{P_{Total} = 7 \ atm}[/tex][tex] \therefore [/tex] The total pressure in the container is 7 atm (D.)
6. Which of the following refers to standard temperature and pressure? 0 atm and 273 K1 atm and 273 K0 atm and 273 degrees C1 atm and 273 degrees C
Answer:
1 atm at 273 k
Explanation:
yan Ang pagkakaalam ko
7. L tank. What is the pressure of the compressed gas, if the temperature remains constant? a. 0.15 atm b. 4.7 atm c. 0.21 atm d. 3.4 atm
3.4 atm because the neutral formula of L is given
8. A confined quantity of gas has a pressure of 2.50 atm and a temperature of -22°C. What is the new pressure if the temperature is increased to 22°C?a. 2.1 atm b. 2.5 atmc. 2.9 atmd. 3.4 atm
ANSWER: C. 2.94 L
According to Charles' Law:
[tex] \frac{pressure1}{temperature1} = \frac{pressure2}{temperature2} [/tex]
Plugging in the terms:
[tex] \frac{2.50}{251} = \frac{x}{295} \\ \frac{2.50(295)}{251} = 2.94[/tex]
The new pressure is 2.9 atm
Hello!
A confined quantity of gas has a pressure of 2.50 atm and a temperature of -22°C. What is the new pressure if the temperature is increased to 22°C ?
a. 2.1 atm
b. 2.5 atm
c. 2.9 atm
d. 3.4 atm
We have an isochoric (isometric or isovolumetric) transformation, it is when a certain mass under pressure maintains its volume constant, if we increase the temperature increases the pressure and if we lower the temperature, the pressure also decreases.
We have the following data:
P1 (initial pressure) = 2.50 atm
T1 (starting temperature) = - 22 ºC (in Kelvin)
TK = TºC + 273.15 → TK = - 22 + 273.15 → TK = 251.15
T1 (starting temperature) = 251.15 K
T2 (final temperature) = 22 ºC (in Kelvin)
TK = TºC + 273.15 → TK = 22 + 273.15 → TK = 295.15
T2 (final temperature) = 295.15 K
P2 (final pressure) = ? (atm)
We apply the data to the formula of isovolumetric transformation (the Second Law of Charles and Gay-Lussac), let us see:
[tex]\dfrac{P_1}{T_1} = \dfrac{P_2}{T_2}[/tex]
[tex]\dfrac{2.50}{251.15} = \dfrac{P_2}{295.15}[/tex]
multiply the means by the extremes
[tex]251.15*P_2 = 2.50*295.15[/tex]
[tex]251.15\:P_2 = 73787.5[/tex]
[tex]P_2 = \dfrac{737.875}{251.15}[/tex]
[tex]P_2 = 2.93798... \to \boxed{\boxed{P_2 \approx 2.9\:atm}}\end{array}}\qquad\checkmark[/tex]
Answer:
c. 2.9 atm
______________________________
I Hope this helps, greetings ... Dexteright02! =)
9. 5. What is the Standard Temperature and Pressure (STP)? A. 1 K, 273 atm B. 100 K, 2 atm C. 273 K 1 atm D. 373 K 1 atm
Answer:
1 atm at 273 k
Explanation:
Answer:
mali yung nasa taas
Explanation:
eto tama sagot wala ako pake
10. At 460C a sample of ammonia gas exerts a pressure of 5.3 atm. What is the pressure when the volume of the gas is reduced to one-tenth (0.10) of the original value at the same temperature? a.53 atm b.71 atm c.45 atm d.67 atm
Answer:
what is the different types of words and cups and cups and mixer accessories for the different options for you and your sentence ☺️ be able and willing and able to do that you something
11. The pressure of a gas is 750 torr when its volume is 400 mL. Calculate the pressure (atm) if the gas is allowed to expand to 600 mL at constant temperature. a. 0.66 atm b. 1.48 atm c. 500 atm d. 1125 atm
Answer:
The answer is letter A.
Explanation:
Given:
P1 = 750 torr
V1 = 400 mL
V2 = 600 mL
P2 =?
Convertion:
1 atm
750 torr x ________ = 0.99 atm (rounded off)
760 torr
1 L
400 mL x ________ = 0.4 L
1000 mL
1 L
600 mL x ________ = 0.6 L
1000 mL
Formula:
V1 P1 = V2 P2
V1 P1
P2 = _____
V2
Solution:
(0.4 L)(0.99 atm)
P2 = ________________
0.6 L
0.39 L atm
P2 = __________
0.6 L
P2 = 0.66 atm
12. A system contrats bya volume of 300 cubic with a pressure of 1.5 atm. Work is equal to
Answer:
Work is equal to - 13785550.
Step-by-step explanation:
no need
13. 7. How many moles of nitrogen are present in the problem?A. 1.05B. 1.06C. 1.07D. 1.088.What is the total moles of the mixture?A. 1.60B. 1.61C. 1. 62D. 1.639. What is the total pressure of the mixture in terms of atm?A. 3.60B. 3.61C. 3.62D. 3.6310. By rearranging the formula for Dalton's law, what is the partial pressure ofoxygen?A. 1.20 atmB. 1.21 atmC. 1.22 atmD. 1.23 atm11. What is the calculated partial pressure of nitrogen?A. 2.40 atmB. 2.41 atmC. 2.42 atmD. 2.43 atmFor items 12-15, refer to this problem: In a laboratory experiment, 98 gof oxygen and 140 g nitrogen are combined in a 5.0 L at 298 K.Calculate for partial pressure of each gas and its total pressure.12. How many moles of oxygen are in the mixture?A. 1.5 molB. 2.5 molC. 3.5 molD. 4.5 mol13. In the problem above, what is the partial pressure of oxygen gas?A. 17.09 atm B. 17.10 atmC. 17.11 atmD. 17.12 atm14. According to the problem, what is partial pressure exerted by a 140 gnitrogen?A. 24.45 atm B. 24.50 atm C. 24.55 atm D. 24.60 atm15. From the given situation, what will be the total pressure of the mixture?A. 41.47 atm B. 41.57 atm C. 41.67 atm D. 41.77 atm
Answer:
7.a
8.b
9.d
10.d
11.b
12.a
13.d
14.a
15.c
14. What phase of water exist at 100°c and 5 atm? at 200°c and 1 atm?
The phase of water that exist at 100°c and 5atm is boiling
15. At 460C a sample of ammonia gas exerts a pressure of 5.3 atm. What is the pressure when the volume of the gas is reduced to one-tenth (0.10) of the original value at the same temperature? a.53 atm b.71 atm c.45 atm d. 67 atm
Answer:
a. 53 ATM po thanks me later if correct
16. pressure to 3.4 atm?A. 1.29 LD. 12.36 atmB. 12.36 LC. 1.29 atm22. If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until its volume is4.8 L, what will the new pressure inside the piston be?4. 1.8 atmB.3.27 atmC. 1.8LD. 3.27 atmUning mu car into the river and it implodes,
22. If you have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until it’s volume
Correct me if I’m wrong this is my answer:
B. 3.27 atm
17. A 10-liter sample of gas is held in a container under a pressure of 1.5 atm. Then gas is then compressed to 7.5 liters. Find the pressure if the temperature is kept unchanged.A. 1.3 atmB. 2.0 atmC. 1.7 atmD. 50 atm
Answer:
B. 2.0 atm
Explanation:
1.5 * 10 = P * 75
18. Which of the following is used as standard pressure in a gas equation? a. 1 atm b. 2 atm c. 3 atm d. 4 atm
Answer:
1 atm is the correct answer
19. At 46C a sample of ammonia gas exerts a pressure of 5.3 atm. What is the pressure when the volume of the gas is reduced to one-tenth (0.10) of the original value at the same temperature? a.53 atm b.71 atm c.45 atm d. 67 atm
Answer:
The answer is A. 53 atm
Explanation:
#CarryonLearningAnswer:A. 53 atmSolution:46 degrees=273+47k=320k=t1=t2Let volume1 of gas be vPressure1 = 5.3atmFor second situationTemperature is sameVolume2=1/10vPressure2=?P1v1/t1=p2v2/t2=5.3*v=?*1/10v= 53 atmHope that this will help you#Trust Me20. each of the following containers has same size. which of following containers has the most compressed gas molecules? A. 10 atm B. 8 atm C. 6 atm D 4 atm
If all the containers have the same size. the answer must be A.A. 10 ATMOSPHERES becoz you will know it
21. Report po pag nonsense and pls explain your answer.. 1. elements and compounds exist as gases at what standard temperature and pressure (stp) A. 1 atm, 25°C B. 1 atm, 26 °C C. 1 atm, 27°C D. 1 atm, 28°C
Answer:
1 atm
Under standard temperature and pressure (STP, or 1 atm and 273 K), a substance which exists as a gas is called a pure gas.
22. a simple of nitrogen occupies 87.0mL at 35•C and 1.1 atm. what will be its volume at 50•C and 4.00 atm
Answer:V2=25.090 mL
Explanation:
23. 4. A sample of neon has a volume of 225 cm at 2 atm of pressure. What will be the pressure of the gas to have a volume of 500 cm? a. 0.2 atm c. 1 atm b. 0.9 atm d. 4 atm
Answer:
Hence, the pressure of the gas that have a volume of 500cm will be 0.9atm (B.)
Step-by-step explanation:
To find out what will be the pressure of a gas that has a volume of 500cm, we must use the Boyle's Equation:
[tex] \boxed{\bold{P_1V_1 = P_2V_2}}[/tex]Since we're finding to the new pressure, we can rewrite the equation:
[tex] \boxed{\bold{P_2 = \frac{V_1P_1}{V_2}}}[/tex]Substitute the given to the formula
[tex] P_2 = \frac{(225)(2)}{500} [/tex][tex] P_2 = \frac{450}{500} [/tex][tex] P_2 \approx 0.9 [/tex]Hence, the pressure of the gas that have a volume of 500cm will be 0.9atm (B.)
24. A gas has an initial pressure and temperature of 70 atm and 350 K, respectively. What is the pressure of a gas at 500 K? a. 200 atm b. 49 atm c. 88 atm d. 100 atm
solution:
[tex] \frac{p1}{p2} = \frac{t1}{t2} \\ \frac{71 \: atm}{p2} = \frac{350k}{500k} \\ p2 = \frac{71atm}{ \frac{350k}{500k} } \\ p2 = 101.4 \: atm[/tex]
so the answet is letter D. which is the closest.
Pls give me feedback! thanks
25. 1. A gas sample has a volume of 13.5 L at a pressure of 1.23 atm and a temperature of 34°C. How much pressure will the gas exert if it is compressed into a 10.5 L container at 45°C? a. 3.64 atm b. 2.64 atm c. 1.64 atm d. 4.64 atm
SOLUTION:
Step 1: List the given values.
To convert the temperature from degree Celsius to kelvin, add 273 to the temperature expressed in degree Celsius.
[tex]\begin{aligned} P_1 & = \text{1.23 atm} \\ V_1 & = \text{13.5 L} \\ T_1 & = 34^{\circ}\text{C} = \text{307 K} \\ V_2 & = \text{10.5 L} \\ T_2 & = 45^{\circ}\text{C} = \text{318 K} \end{aligned}[/tex]
Step 2: Calculate the final pressure using combined gas law.
[tex]\begin{aligned} P_2 & = \frac{P_1V_1T_2}{V_2T_1} \\ & = \frac{(\text{1.23 atm})(\text{13.5 L})(\text{318 K})}{(\text{10.5 L})(\text{307 K})} \\ & = \boxed{\text{1.64 atm}} \end{aligned}[/tex]
Hence, the answer is c. 1.64 atm.
[tex]\\[/tex]
#CarryOnLearning
26. Report po pag nonsense and pls explain your answer..1. elements and compounds exist as gases at what standard temperature and pressure (stp) A. 1 atm, 25°C B. 1 atm, 26 °CC. 1 atm, 27°CD. 1 atm, 28°C
Answer:
Under standard temperature and pressure (STP, or 1 atm and 273 K), a substance which exists as a gas is called a pure gas.
27. 1. A gas sample has a volume of 13.5 L at a pressure of 1.23 atm and a temperature of 34°C. How much pressure will the gas exert if it is compressed into a 10.5 L container at 45°C? a. 3.64 atm b. 2.64 atm c. 1.64 atm d. 4.64 atm
Answer:
c. 1.64 atm
Explanation:
((1.23)(13.5))/273+34 = ((x)(10.5))/273+45
shift solve
=1.6381 atm = 1.64 atm
28. A container holds 600 mL of Helium gas at a constant temperature and a pressure of 1.8 atm. What will be the pressure if the volume decreased to 350 mL? A. 3.58 atm B. 3.09 atm C. 0.8 atm D. 1.96 atm
SOLUTION:
Step 1: List the given values.
[tex]\begin{aligned} P_1 & = \text{1.8 atm} \\ V_1 & = \text{600 mL} \\ V_2 & = \text{350 mL} \end{aligned}[/tex]
Step 2: Calculate the final pressure by using Boyle's law.
[tex]\begin{aligned} P_2 & = \frac{P_1V_1}{V_2} \\ & = \frac{(\text{1.8 atm})(\text{600 mL})}{\text{350 mL}} \\ & = \boxed{\text{3.09 atm}} \end{aligned}[/tex]
Hence, the answer is B. 3.09 atm
[tex]\\[/tex]
#CarryOnLearning
29. 800. mL of helium is at 55.0ºC and 0.55 atm. What will the pressure be if the temperature changes to 100.ºC if the volume remains the same? a. 1 atm b. 0.62 atm c. 0.48 atm d. 0.75
The pressure if the temperature changes to 100 ºC : 1 atm
Further explanationGay-Lussac's Law states that the pressure of a gas proportional to its absolute temperature of the gas when the volume is kept constant
The equation can be written :
[tex]\rm \dfrac{P_1}{T_1}=\dfrac{P_2}{T_2}[/tex]
800. mL of helium is at 55.0ºC and 0.55 atm
temperature changes to 100.ºC
So :
V (constant) = 800 ml
T1 = 55.0ºC
P1 = 0.55 atm
T2 = 100.ºC
Then :
[tex]\rm P_2=\dfrac{P_1\times T_2}{T_1}\\\\P_2=\dfrac{0.55\times 100}{55}\\\\P_2=\boxed{\bold{1~atm}}[/tex]
Learn moreExample of ideal gas law in real life
brainly.ph/question/2117053
Example Problem And solution Of combined gas laws
brainly.ph/question/2143722
applications involving combined gas law
brainly.ph/question/2341366
#LetsStudy
30. 1. If oxygen exerts a 4atm of pressure in a mixture and the total pressure of the system is 10 atm, what would be the mole fraction of oxygen in the mixture? 2. Compute for the mole fraction of neon exerting a pressure of 0.28 atm in a gas mixture which has a total pressure of 1.15 atm. 3. If neon exerts 10 atm of pressure in a mixture and the total pressure of the system is 28 atm, what would be the mole fraction of neon in the mixture? Nonsense answer = report
Answer:
0.4
Explanation:
For example, if oxygen exerts 4 atm of pressure in a mixture and the total pressure of the system is 10 atm, the mole ratio would be 4/10 or 0.4. The mole ratio applies to pressure, volume, and moles as seen by the equation below. This also means that 0.4 moles of the mixture is made up of gas
Answer:
1.
0.4
2.
0.25 atm
3.
280
Explanation:
