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One mole of hydrogen gas is heated at constant pressure from 300 K to 420 K. Calculate the energy transferred by heat to the gas
- a)3.86 kJ
- b)3.49 kJ
- c)3.66 kJ
- d)3.26 kJ
Correct answer is option 'B'. Can you explain this answer?
Verified Answer
One mole of hydrogen gas is heated at constant pressure from 300 K to ...
Explanation:
Hydrogen is a diatomic gas. (CP = 3.5R)
energy transferred by heat to the gas
Q=nCPΔT=1×3.5×8.31×120=3490J=3.49KJ
Most Upvoted Answer
One mole of hydrogen gas is heated at constant pressure from 300 K to ...
To calculate the energy transferred by heat to the gas, we can use the formula:
q = nCΔT
Where:
q = energy transferred by heat
n = number of moles of gas
C = molar heat capacity at constant pressure
ΔT = change in temperature
Given:
n = 1 mole
ΔT = 420 K - 300 K = 120 K
We need to find the value of C, the molar heat capacity at constant pressure.
The molar heat capacity at constant pressure (Cp) for an ideal gas can be calculated using the equation:
Cp = 5/2R
Where:
R = ideal gas constant = 8.314 J/mol·K
Substituting the values, we have:
Cp = 5/2 * 8.314 J/mol·K = 20.785 J/mol·K
Now, we can substitute the values of n, C, and ΔT into the formula:
q = (1 mole)(20.785 J/mol·K)(120 K)
q = 2494.2 J
To convert the energy from joules to kilojoules, we divide by 1000:
q = 2494.2 J / 1000 = 2.4942 kJ
Therefore, the energy transferred by heat to the gas is approximately 2.4942 kJ. None of the given options matches this value, so we need to consider significant figures.
The given temperature values are given to three significant figures (300 K and 420 K). Therefore, our final answer should also be rounded to three significant figures.
Rounding 2.4942 kJ to three significant figures, we get:
2.49 kJ
Among the given options, option B, 3.49 kJ, is the closest match to our rounded answer.
q = nCΔT
Where:
q = energy transferred by heat
n = number of moles of gas
C = molar heat capacity at constant pressure
ΔT = change in temperature
Given:
n = 1 mole
ΔT = 420 K - 300 K = 120 K
We need to find the value of C, the molar heat capacity at constant pressure.
The molar heat capacity at constant pressure (Cp) for an ideal gas can be calculated using the equation:
Cp = 5/2R
Where:
R = ideal gas constant = 8.314 J/mol·K
Substituting the values, we have:
Cp = 5/2 * 8.314 J/mol·K = 20.785 J/mol·K
Now, we can substitute the values of n, C, and ΔT into the formula:
q = (1 mole)(20.785 J/mol·K)(120 K)
q = 2494.2 J
To convert the energy from joules to kilojoules, we divide by 1000:
q = 2494.2 J / 1000 = 2.4942 kJ
Therefore, the energy transferred by heat to the gas is approximately 2.4942 kJ. None of the given options matches this value, so we need to consider significant figures.
The given temperature values are given to three significant figures (300 K and 420 K). Therefore, our final answer should also be rounded to three significant figures.
Rounding 2.4942 kJ to three significant figures, we get:
2.49 kJ
Among the given options, option B, 3.49 kJ, is the closest match to our rounded answer.
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One mole of hydrogen gas is heated at constant pressure from 300 K to 420 K. Calculate the energy transferred by heat to the gasa)3.86 kJb)3.49kJc)3.66 kJd)3.26 kJCorrect answer is option 'B'. Can you explain this answer? for Class 11 2025 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about One mole of hydrogen gas is heated at constant pressure from 300 K to 420 K. Calculate the energy transferred by heat to the gasa)3.86 kJb)3.49kJc)3.66 kJd)3.26 kJCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for One mole of hydrogen gas is heated at constant pressure from 300 K to 420 K. Calculate the energy transferred by heat to the gasa)3.86 kJb)3.49kJc)3.66 kJd)3.26 kJCorrect answer is option 'B'. Can you explain this answer?.
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