1. As the temperature of the gas in a balloon decreases, which of the following occurs? The volume of the balloon increases. ***
2 answers:
Answer 1:
Correct Answer: T<span>he average kinetic energy of the gas decreases.
</span>Reason:
From the ideal gas equation, we know that PV = nRT
where, P = pressure, V = volume, n = number of moles of gas, R = gas constant and T = temperature.
From above equation, it can be seen that, Temp. as a direct relation with Pressure and Volume. Hence, as temperature of the gas in a balloon decreases, pressure and volume also decreases.
Also, from kinetic theory of gases, we know that, kinetic energy of gas increases with increasing temp. Hence, average kinetic energy of the gas decreases with decreasing temp.
Answer 2:
Correct answer: Out
Reason:
From the ideal gas equation, we know that PV = nRT
where, P = pressure, V = volume, n = number of moles of gas, R = gas constant and T = temperature.
Therefore, when a sealed syringe is heated, it's temp. will increase. This, will result in expansion of gas i.e volume will increase. Hence, <span>syringe plunger move in outwards direction.
Answer 3: Volume = 6046 L
Reason:
</span>From the ideal gas equation, we know that PV = RT
where, P = pressure, V = volume, R = gas constant and T = temperature.<span>
Given: P1 = 99 kPa, V1 = 3000 L, T1 = 312 K, P2 = 45.5 KPa and T2 = 289 K.
Therefore, we have: </span>
Thus,
Hence, V2 = 6046 L
Answer 4:
Correct Answer: It increases
Reason:
We know that, pressure of gas, it directly proportional to temp. Hence, when the temp. of as is increases. Total pressure of gas mixture increases. This is because, partial pressure of individual component (in present case oxygen) increases.
Answer 5:
Correct answer: 18.5 kPa
Reason:
We know that, total pressure is the sum of the partial pressures of the gases present in it. Mathematically, it can be expressed as:
Ptot = PO2 + PHe + PCO2
Correct Answer: T<span>he average kinetic energy of the gas decreases.
</span>Reason:
From the ideal gas equation, we know that PV = nRT
where, P = pressure, V = volume, n = number of moles of gas, R = gas constant and T = temperature.
From above equation, it can be seen that, Temp. as a direct relation with Pressure and Volume. Hence, as temperature of the gas in a balloon decreases, pressure and volume also decreases.
Also, from kinetic theory of gases, we know that, kinetic energy of gas increases with increasing temp. Hence, average kinetic energy of the gas decreases with decreasing temp.
Answer 2:
Correct answer: Out
Reason:
From the ideal gas equation, we know that PV = nRT
where, P = pressure, V = volume, n = number of moles of gas, R = gas constant and T = temperature.
Therefore, when a sealed syringe is heated, it's temp. will increase. This, will result in expansion of gas i.e volume will increase. Hence, <span>syringe plunger move in outwards direction.
Answer 3: Volume = 6046 L
Reason:
</span>From the ideal gas equation, we know that PV = RT
where, P = pressure, V = volume, R = gas constant and T = temperature.<span>
Given: P1 = 99 kPa, V1 = 3000 L, T1 = 312 K, P2 = 45.5 KPa and T2 = 289 K.
Therefore, we have: </span>
Thus,
Hence, V2 = 6046 L
Answer 4:
Correct Answer: It increases
Reason:
We know that, pressure of gas, it directly proportional to temp. Hence, when the temp. of as is increases. Total pressure of gas mixture increases. This is because, partial pressure of individual component (in present case oxygen) increases.
Answer 5:
Correct answer: 18.5 kPa
Reason:
We know that, total pressure is the sum of the partial pressures of the gases present in it. Mathematically, it can be expressed as:
Ptot = PO2 + PHe + PCO2
Therefore, partial pressure of oxygen, <span>PO2:</span>
PO2 = Ptot − PHe − PCO2
= 101.4 − 82.5 − 0.4
=18.5 kPa.
Answer 6:
Correct Answer: Argon
Reason:
<span>Inert gases are the best choice for inflating a balloon that must remain inflated for a long period of time. Among given options, both neon and argon are inert gas, But, atomic weight of Ar is 40g/mol, while is more than that of neon (20 g/mol). Hence,. Argon gas is preferred over neon gas. </span>You might be interested in
<span>Molar mass (MM) of benzene C6H6
C = 6 * 12 = 72u
H = 6 * 1 = 6u
MM C6H6 = 72 + 6 = 78 g / mol
Benzene - Molar Mass = 78 g --------- 1 mol
Of A Mix has 468 g -------------- x
78x = 468
X = 468/78
X = 6 moles
Molar mass (MM) of Hydrochloric Acid HCl H = 1 * 1 = 1u
CI = 1 * 35 = 35u
MM HCl = 1 + 35 = 36 g / mol
Hydrochloric Acid - Molar Mass = 36 g ---------- 1 mol
Of A Mix has 72 g ------------ y
36y = 72
Y = 72/36
Y = 2 moles
Thus, a mixture has a total of 8 moles (6 mol + 2 mol).
Dividing One Mole Amount of Each Substance by the Number of Total Mole Amounts, Then we will obtain a Molar Fraction of Each:
Molar fraction make benzene = (6/8) simplify 2 = 3/4
Molar Fraction to make Hydrochloric Acid = (2/8) = simplify 2 = 1/4
Note:. The sum of the molar fractions of the always give goes 1, we have: 3/4 + 1/4 = 1
ANSWER:
</span>
C = 6 * 12 = 72u
H = 6 * 1 = 6u
MM C6H6 = 72 + 6 = 78 g / mol
Benzene - Molar Mass = 78 g --------- 1 mol
Of A Mix has 468 g -------------- x
78x = 468
X = 468/78
X = 6 moles
Molar mass (MM) of Hydrochloric Acid HCl H = 1 * 1 = 1u
CI = 1 * 35 = 35u
MM HCl = 1 + 35 = 36 g / mol
Hydrochloric Acid - Molar Mass = 36 g ---------- 1 mol
Of A Mix has 72 g ------------ y
36y = 72
Y = 72/36
Y = 2 moles
Thus, a mixture has a total of 8 moles (6 mol + 2 mol).
Dividing One Mole Amount of Each Substance by the Number of Total Mole Amounts, Then we will obtain a Molar Fraction of Each:
Molar fraction make benzene = (6/8) simplify 2 = 3/4
Molar Fraction to make Hydrochloric Acid = (2/8) = simplify 2 = 1/4
Note:. The sum of the molar fractions of the always give goes 1, we have: 3/4 + 1/4 = 1
ANSWER:
</span>