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The gas with an initial volume of 24.0 L at a pressure of 565 mmHg is compressed until the volume is 16.0 L What is the final pressure of the gas?
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∙ 11y ago
500. mmHg
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∙ 11y ago
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A gas is compressed from an initial volume of 5.75 to a final volume of 1.21 by an external pressure of 1.00 During the compression the gas releases 121 of heat?
121
What happens to the volume of solids liquids and gases when they cool?
Solids- stays the same Liquids- stays the same Gases- decreases You can use the formula PV/T=P2V2/T2 P=initial pressure V=initial volume T=initial temp P2=final pressure V2=final volume T2=final temp
What will the pressure inside the container become if the piston is moved to the 1.80 L rm L mark while the temperature of the gas is kept constant?
This problem can be solved with the ideal gas law. The original pressure and volume of the container are proportional the final pressure and volume of the container. The original pressure was 1 atmosphere and the original volume was 1 liter. If the final volume is 1.8 liters, then the final pressure is 0.55 atmospheres.
What does equation V1 c1 v2 c2 stand for where c concentration and v is for volume?
v1= initial volume c1= initial concentration v2= final volume c2= final concentration For example, you have 10mL of an unknown substance with a concentration of 0,5mol/L. If you add 50mL, what will the final concentration be. V1= 10mL C1= 0,5mol/L V2= 60mL C2= x 10/0,5=60/x You must start by putting everything in the same mesure. We'll use mL here. So 0,5-->1000mL= 50-->10mL 50x60= 300 300/10= 30 30 is your C2
What is the concentration of a solution prepared by diluting 20.0mL of a 0.200 M NaCl to 250.0 mL?
Use the equation M(initial)*V(initial)=M(final)*V(final). In this case, M(initial) is 0.200 M NaCl. V(initial) is 20.0mL. V(final) is 250.0mL. You are solving for M(final). To solve, you rearrange the equation so M(final)=(M(initial)*V(initial))/V(final), which gives you (0.200*20.0)/250. The answer is 0.016 M for M(final). You don't need to convert mL to L in this type of problem. You can if you want, but you will end up with the same answer. It's just an extra unnecessary step, unless the question is asking for a Volume in L. But in this case you were asked for concentration (Molarity), so no volume conversions were necessary.
What happened to the pressure when air was compressed?
When air is compressed at the same temperate and volume space, pressure will increase in accordance with Boyle's Law which states: PV/T (initial) = PV/T (final) where P is pressure, V is volume and T is temperature.
A gas is compressed from an initial volume of 5.75 to a final volume of 1.21 by an external pressure of 1.00 During the compression the gas releases 121 of heat?
121
What is Charles law and boyles law?
BOYLES LAW The relationship between volume and pressure. Remember that the law assumes the temperature to be constant. or V1 = original volume V2 = new volume P1 = original pressure P2 = new pressure CHARLES LAW The relationship between temperature and volume. Remember that the law assumes that the pressure remains constant. V1 = original volume T1 = original absolute temperature V2 = new volume T2 = new absolute temperature P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature IDEAL GAS LAW P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature Answer BOYLES LAW The relationship between volume and pressure. Remember that the law assumes the temperature to be constant. or V1 = original volume V2 = new volume P1 = original pressure P2 = new pressure CHARLES LAW The relationship between temperature and volume. Remember that the law assumes that the pressure remains constant. V1 = original volume T1 = original absolute temperature V2 = new volume T2 = new absolute temperature P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature IDEAL GAS LAW P1 = Initial Pressure V1= Initial Volume T1= Initial Temperature P2= Final Pressure V2= Final Volume T2= Final Temperature
How to calculate final pressure when given initial pressure and initial temp and also final temp and know that it's a constant volume process from initial state?
You can calculate pressure and temperature for a constant volume process using the combined gas law.
What happens to the volume of solids liquids and gases when they cool?
Solids- stays the same Liquids- stays the same Gases- decreases You can use the formula PV/T=P2V2/T2 P=initial pressure V=initial volume T=initial temp P2=final pressure V2=final volume T2=final temp
What happens when a gas is compressed keeping the temperature constant?
If pressure is held constant, volume and temperature are directly proportional. That is, as long as pressure is constant, if volume goes up so does temperature, if temperature goes down so does volume. This follows the model V1/T1=V2/T2, with V1 as initial volume, T1 as initial temperature, V2 as final volume, and T2 as final temperature.
What must the pressure and volume be if the pressure of its container is reduced to half its original size?
initial volume = V1 final volume = V2 initial pressure = P1 final pressure = P2 = (1/2)P1 P1V1 = P2V2 P1V1 = (1/2)P1V2 P1 cancels; V1 = (1/2)V2 V2 = 2V2.
What is the final pressure of a system (ATM) that has the volume increased from 0.75 L to 3.1L with an initial pressure of 1.25 ATM?
1.1
If 20.00mL of a 1.50M solution of KBr is diluted to a final volume of 150.0mL what is the new molar concentration?
initial molarity*initial volume= final molarity*final volume Initial molarity= 1.50M Initial volume= 20.00ml Final Volume=150.0ml Thus final molarity =1.50M*20ml/150ml=0.200M. New molar concentration= final molarity
How do you find the volume of a displaced object when the initial and final volumes are shown?
Subtract the initial from the final
What is the final volume of a gas with an initial volume of 75 mL if the pressure decreases from 300 m to 200 mL?
What? Pressure cannot be measured in m or in mL. Please check you homework and resubmit the correct question.
500cm3 of ideal gas at 40 degrees Celsius and 200kpa absolute is compressed to 250cm3 and cooled to 20 degrees Celsius.What is the final absolute pressure?
Assuming the amount of gas remains constant, we can use the ideal gas law to calculate the final absolute pressure. The initial pressure (P1) is 200 kPa and the final volume (V2) is 250 cm3. The initial temperature (T1) is 40 degrees Celsius or 313.15 Kelvin, and the final temperature (T2) is 20 degrees Celsius or 293.15 Kelvin. Using the equation (P1 * V1) / T1 = (P2 * V2) / T2, we can solve for the final absolute pressure (P2), which is approximately 400 kPa.
